Question 11 Mark
Which of the following reactions will get affected by increasing the pressure? Also, mention whether change will cause the reaction to go into forward or backward direction.
$\text{2H}_2\text{ (g) + CO}\text{ (g)}\rightleftharpoons\text{CH}_3\text{OH (g)}$
AnswerOnly those reactions will be affected by increasing the pressure in which the number of moles of the gaseous reactants and products are different (n
p ≠ n
r) (gaseous). With the exception of the reaction (1); all the reamaining five reactions will get affected by increasing the pressure. In general,
- The reaction will go to the left if np > nr.
- The reaction will go to the right if nr > np.
Keeping this in mind,
Increase in pressure will favour forward reaction because n
p (1) < n
r (2)
View full question & answer→Question 21 Mark
Does the number of moles of reaction products increase, decrease or remain same when each of the following equilibria is subjected to a decrease in pressure by increasing the volume?
$\text{3Fe}\text{ (S) + }\text{4H}_2\text{O (g)}\rightleftharpoons\text{Fe}_3\text{O}_4\text{ (S) + 4H}_2\text{ (g)}$
AnswerThe number of moles of reaction products remains the same.
View full question & answer→Question 31 Mark
Predict if the solutions of the following salts are neutral, acidic or basic:
NaCN
Answer | $\text{NaCN}$ | $+$ | $\text{H}_2\text{O}$ | $\leftrightarrow$ | $\text{HCN}$ | $+$ | $\text{NaOH}$ |
| | | | | $\text{Weak acid}$ | | $\text{Strong base}$ |
Therefore, it is a basic solution.
View full question & answer→Question 41 Mark
Predict if the solutions of the following salts are neutral, acidic or basic:
NH4NO3
Answer | $\text{NH}_4\text{NO}_3$ | $+$ | $\text{H}_2\text{O}$ | $\leftrightarrow$ | $\text{NH}_4\text{OH}$ | $+$ | $\text{HNO}_3$ |
| | | | | $\text{Weak base}$ | | $\text{Strong acid}$ |
Therefore, it is an acidic solution.
View full question & answer→Question 51 Mark
Predict if the solutions of the following salts are neutral, acidic or basic:
KBr
Answer | $\text{KBr}$ | $+$ | $\text{H}_2\text{O}$ | $\leftrightarrow$ | $\text{KOH}$ | $+$ | $\text{HBr}$ |
| | | | | $\text{Strong base}$ | | $\text{Strong acid}$ |
Therefore, it is a neutral solution.
View full question & answer→Question 61 Mark
Predict if the solutions of the following salts are neutral, acidic or basic:
KF
Answer | $\text{KF}$ | $+$ | $\text{H}_2\text{O}$ | $\leftrightarrow$ | $\text{KOH}$ | $+$ | $\text{HF}$ |
| | | | | $\text{Strong base}$ | | $\text{weak acid}$ |
Therefore, it is a basic solution.
View full question & answer→Question 71 Mark
Does the number of moles of reaction products increase, decrease or remain same when each of the following equilibria is subjected to a decrease in pressure by increasing the volume?
$\text{CaO}\text{ (S) + }\text{CO}_2\text{ (g)}\rightleftharpoons\text{CaCO}_3\text{ (S)}$
AnswerThe number of moles of reaction products will decrease.
View full question & answer→Question 81 Mark
A liquid is in equilibrium with its vapour in a sealed container at a fixed temperature. The volume of the container is suddenly increased.
What is the initial effect of the change on vapour pressure?
AnswerOn increasing the volume of the container, the vapour pressure will initially decrease because the same amount of vapours are now distributed over a larger space.
View full question & answer→Question 91 Mark
What is Kc for the following equilibrium when the equilibrium concentration of each substance is:
[SO2]= 0.60M, [O2] = 0.82M and [SO3] = 1.90M?
2SO2(g) + O2(g) ⇌ 2SO3(g)
Answer2SO2(g) + O2(g) ⇌ 2SO3(g)
Applying law of chemical equilibrium.
View full question & answer→Question 101 Mark
Calculate the hydrogen ion concentration in the following biological fluids whose pH are given below:
Human blood, 7.38
AnswerHuman blood, 7.38:
$\text{pH}=7.38=-\log[\text{H}^+]$
$\therefore\ [\text{H}^+]=4.17\times10^{-8}\text{M}$
View full question & answer→Question 111 Mark
Predict if the solutions of the following salts are neutral, acidic or basic:
NaNO2
Answer | $\text{NaNO}_2$ | $+$ | $\text{H}_2\text{O}$ | $\leftrightarrow$ | $\text{Na}\text{OH}$ | $+$ | $\text{HNO}_2$ |
| | | | | $\text{Strong base}$ | | $\text{weak acid}$ |
Therefore, it is a basic solution.
View full question & answer→Question 121 Mark
Predict if the solutions of the following salts are neutral, acidic or basic:
NaCl
Answer | $\text{NaCl}$ | $+$ | $\text{H}_2\text{O}$ | $\leftrightarrow$ | $\text{NaOH}$ | $+$ | $\text{HCl}$ |
| | | | | $\text{Strong base}$ | | $\text{Strong acid}$ |
Therefore, it is a neutral solution.
View full question & answer→Question 131 Mark
For the following equilibrium, $\text{K}_{\text{c}}=6.3\times10^{14}\text{ at }1000\text{K}$
$\text{NO(g) + O}_3\text{(g)}\rightleftharpoons\text{NO}_2\text{(g) + O}_2\text{(g)}$
Both the forward and reverse reactions in the equilibrium are elementary bimolecular reactions. What is Kc, for the reverse reaction?
AnswerFor the reverse reaction $\text{K}_{\text{c}}=\frac{1}{\text{K}_{\text{c}}}=\frac{1}{6.3\times10^{14}}=1.59\times10^{-15.}$
View full question & answer→Question 141 Mark
What will be the conjugate bases for the Brönsted acids: HF, H2SO4 and $\text{HCO}_3^-$?
AnswerThe table below lists the conjugate bases for the given Bronsted acids.
| $\text{Bronsted acid Conjugate base}$ |
| $\text{HF}$ | $\text{F}^-$ |
| $\text{H}_2\text{SO}_4$ | $\text{HSO}_4^-$ |
| $\text{HCO}_3^-$ | $\text{CO}_3^{2-}$ |
View full question & answer→Question 151 Mark
Which of the following reactions will get affected by increasing the pressure? Also, mention whether change will cause the reaction to go into forward or backward direction.
$\text{4NH}_3\text{ (g) + 5O}_2\text{ (g)}\rightleftharpoons\text{4NO}\text{ (g) + 6H}_2\text{O (g)}$
AnswerOnly those reactions will be affected by increasing the pressure in which the number of moles of the gaseous reactants and products are different (n
p ≠ n
r) (gaseous). With the exception of the reaction (1); all the reamaining five reactions will get affected by increasing the pressure. In general,
- The reaction will go to the left if np > nr.
- The reaction will go to the right if nr > np.
Keeping this in mind,
Increase in pressure will favour backward reaction because n
p (1) > n
r (0).
View full question & answer→Question 161 Mark
Calculate the hydrogen ion concentration in the following biological fluids whose pH are given below:
Human muscle-fluid, 6.83
AnswerHuman muscle fluid 6.83:
$\text{pH}=6.83$
$\text{pH}=-\log\text{[H}^+]$
$\therefore\ 6.83=-\log[\text{H}^+]$
$[\text{H}^+]=1.48\times10^{-7}\text{M}$
View full question & answer→Question 171 Mark
Predict which of the following reaction will have appreciable concentration of reactants and products:
$\text{Cl}_2\text{ (g)}+\text{2NO}_2\text{ (g)}\rightleftharpoons2\text{NO}_2\text{Cl (g) K}_\text{c}=1.8$
AnswerFollowing conclusions can be drawn from the values of Kc.
Since the value of Kc is 1.8, this means that both the products and reactants have appreciable concentration.
View full question & answer→Question 181 Mark
Write the expression for the equilibrium constant, Kc for each of the following reactions:
$\text{I}_2\text{(S)}+5\text{F}_2\rightleftharpoons2\text{IF}_5$
Answer$\text{K}_{\text{c}}=\frac{[\text{IF}_5\text{(l)}]^2}{[\text{l}_2\text{(S)}][\text{F}_2\text{(g)}]^5}$
$=\frac{[\text{IF}_5\text{(l)}]^2}{[\text{F}_2\text{(g})']^5}$
View full question & answer→Question 191 Mark
Which of the following reactions will get affected by increasing the pressure? Also, mention whether change will cause the reaction to go into forward or backward direction.
$\text{COCl}_2\text{ (g)}\rightleftharpoons\text{CO (g) + Cl}_2\text{ (g)}$
AnswerOnly those reactions will be affected by increasing the pressure in which the number of moles of the gaseous reactants and products are different (n
p ≠ n
r) (gaseous). With the exception of the reaction (1); all the reamaining five reactions will get affected by increasing the pressure. In general,
- The reaction will go to the left if np > nr.
- The reaction will go to the right if nr > np.
Keeping this in mind,
Increase in pressure will not affect equilibrium because n
p = n
r = 3.
View full question & answer→Question 201 Mark
Ethyl acetate is formed by the reaction between ethanol and acetic acid and the equilibrium is represented as:
$\text{CH}_3\text{COOH (1) + C}_2\text{H}_5\text{OH (1)}\rightleftharpoons\text{CH}_3\text{COOC}_2\text{H}_5 \text{ (1) + H}_2\text{O (1)}$
Write the concentration ratio (reaction quotient), Qc, for this reaction (note: water is not in excess and is not a solvent in this reaction)
AnswerReaction quotient,$\text{Q}_{\text{c}}=\frac{[\text{CH}_3\text{COOC}_2\text{H}_5][\text{H}_2\text{O]}}{[\text{CH}_3\text{COOH][}\text{C}_2\text{H}_5\text{OH}] }$
View full question & answer→Question 211 Mark
Predict which of the following reaction will have appreciable concentration of reactants and products:
$\text{Cl}_2\text{ (g)}\rightleftharpoons2\text{Cl (g) K}_\text{c}=5\times10^{-39}$
AnswerFollowing conclusions can be drawn from the values of Kc.
Since the value of Kc is very small, this means that the molar concentration of the products is very small as compared to that of the reactants.
View full question & answer→Question 221 Mark
Which of the following reactions will get affected by increasing the pressure? Also, mention whether change will cause the reaction to go into forward or backward direction.
$\text{CaCO}_3\text{ (S)}\rightleftharpoons\text{CaO}\text{ (S) + CO}_2\text{ (g)}$
AnswerOnly those reactions will be affected by increasing the pressure in which the number of moles of the gaseous reactants and products are different (n
p ≠ n
r) (gaseous). With the exception of the reaction (1); all the reamaining five reactions will get affected by increasing the pressure. In general,
- The reaction will go to the left if np > nr.
- The reaction will go to the right if nr > np.
Keeping this in mind,
Increase in pressure will favour backward reaction because n
p (2) > n
r(1)
View full question & answer→Question 231 Mark
Which of the following reactions will get affected by increasing the pressure? Also, mention whether change will cause the reaction to go into forward or backward direction.
$\text{CO}_2\text{ (g) + C}\text{ (S)}\rightleftharpoons\text{2CO}\text{ (g)}$
AnswerOnly those reactions will be affected by increasing the pressure in which the number of moles of the gaseous reactants and products are different (n
p ≠ n
r) (gaseous). With the exception of the reaction (1); all the reamaining five reactions will get affected by increasing the pressure. In general,
- The reaction will go to the left if np > nr.
- The reaction will go to the right if nr > np.
Keeping this in mind,
Increase in pressure will favour backward reaction because n
p (10) > n
r (9)
View full question & answer→Question 241 Mark
Describe the effect of:
addition of H2
on the equilibrium of the reaction:
$2\text{H}_2\text{ (g) + CO (g)}\rightleftharpoons\text{CH}_3\text{OH (g)}$
AnswerAccording to Le Chatelier’s principle, on addition of H2, the equilibrium of the given reaction will shift in the forward direction.
View full question & answer→Question 251 Mark
At 473K, equilibrium constant Kc for decomposition of phosphorus pentachloride, PCl5 is 8.3 ×10-3. If decomposition is depicted as,
$\text{PCl}_5\text{ (g)}\rightleftharpoons\text{PCl}_3\text{ (g) + Cl}_2\text{ (g)}\ \Delta_\text{r}\text{H}^\ominus=124.0\text{ kJ mol}^{-1}$
what would be the effect on Kc if
- more PCl5 is added
- pressure is increased
- the temperature is increased?
Answer$\text{PCl}_{5\text{(g)}}\rightleftharpoons\text{PCl}_{3\text{(g)}}+\text{Cl}_{2\text{(g)}}$
- If more $\text{PCl}_5$ is added, then $\text{Q}_\text{c}$ becomes less than $\text{K}_{\text{c}'}$ the reaction will shift in the forward direction.
- If the pressure is increased, the reaction will shift towards backward direction as it contains less number of gaseous species. $\text{K}_\text{c}$ remains constant.
- As the reaction is endothermic, the increase in temperature will favour the forward reaction. More $\text{PCl}_5$ will dissociate to form $\text{PCl}_3$ and $\text{Cl}_2.$ $\text{K}_\text{c}$ increases.
View full question & answer→Question 261 Mark
Predict which of the following reaction will have appreciable concentration of reactants and products:
$\text{Cl}_2\text{ (g)}+\text{2NO (g)}\rightleftharpoons2\text{NOCl (g) K}_\text{c}=3.7\times10^8$
AnswerFollowing conclusions can be drawn from the values of Kc.
Since the value of Kc is quite large, this means that the molar concentration of the products is very large as compared to that of the reactants.
View full question & answer→Question 271 Mark
At 473K, equilibrium constant Kc for decomposition of phosphorus pentachloride, PCl5 is 8.3 ×10-3. If decomposition is depicted as,
$\text{PCl}_5\text{ (g)}\rightleftharpoons\text{PCl}_3\text{ (g) + Cl}_2\text{ (g)}\ \Delta_\text{r}\text{H}^\ominus=124.0\text{ kJ mol}^{-1}$
write an expression for Kc for the reaction.
Answer$\text{K}_\text{c}=\frac{[\text{PCl}_{3\text{(g)}}][\text{Cl}_{2\text{(g)}}]}{[\text{PCl}_{5\text{(g)}}]}$
View full question & answer→Question 281 Mark
At 473K, equilibrium constant Kc for decomposition of phosphorus pentachloride, PCl5 is 8.3 ×10-3. If decomposition is depicted as,
$\text{PCl}_5\text{ (g)}\rightleftharpoons\text{PCl}_3\text{ (g) + Cl}_2\text{ (g)}\ \Delta_\text{r}\text{H}^\ominus=124.0\text{ kJ mol}^{-1}$
what is the value of Kc for the reverse reaction at the same temperature?
Answer$\text{PCl}_{3\text{(g)}}+\text{Cl}_{2\text{(g)}}\rightleftharpoons\text{PCl}_{5\text{(g)}}$
$\therefore\ \text{K}'_\text{c}=\frac{[\text{PCl}_{5\text{(g)}}]}{[\text{PCl}_{3\text{(g)}}][\text{Cl}_{2\text{(g)}}]}=\frac{1}{8.3\times10^{-3}}=120.48$
View full question & answer→Question 291 Mark
Which of the following reactions will get affected by increasing the pressure? Also, mention whether change will cause the reaction to go into forward or backward direction.
$\text{CH}_4\text{ (g) + 2S}_2\text{ (g)}\rightleftharpoons\text{CS}_2\text{ (g) + 2H}_2\text{S}\text{ (g)}$
AnswerOnly those reactions will be affected by increasing the pressure in which the number of moles of the gaseous reactants and products are different (n
p ≠ n
r) (gaseous). With the exception of the reaction (1); all the reamaining five reactions will get affected by increasing the pressure. In general,
- The reaction will go to the left if np > nr.
- The reaction will go to the right if nr > np.
Keeping this in mind,
Increase in pressure will favour backward reaction because n
p (2) > n
r (1)
View full question & answer→Question 301 Mark
Write the conjugate acids for the following Brönsted bases: $\text{NH}_2^-$, NH3 and HCOO–.
AnswerThe table below lists the conjugate acids for the given Bronsted bases.
| $\text{Bronsted base Conjugate acid}$ |
| $\text{NH}_2^-$ | $\text{NH}_3$ |
| $\text{NH}_3$ | $\text{NH}_4^+$ |
| $\text{HCOO}^-$ | $\text{HCOOH}$ |
View full question & answer→Question 311 Mark
Calculate the hydrogen ion concentration in the following biological fluids whose pH are given below:
Human stomach fluid, 1.2
AnswerHuman stomach fluid, 1.2:
$\text{pH}=1.2$
$1.2=-\log[\text{H}^+]$
$\therefore\ [\text{H}^+]=0.063$
View full question & answer→Question 321 Mark
Describe the effect of:
removal of CH3OH
on the equilibrium of the reaction:
$2\text{H}_2\text{ (g) + CO (g)}\rightleftharpoons\text{CH}_3\text{OH (g)}$
AnswerOn removing CH3OH, the equilibrium will shift in the forward direction.
View full question & answer→Question 331 Mark
Calculate the hydrogen ion concentration in the following biological fluids whose pH are given below:
Human saliva, 6.4.
AnswerHuman saliva, 6.4:
$\text{pH}=6.4$
$6.4=-\log[\text{H}^+]$
$[\text{H}^+]=3.98\times10^{-7}$
View full question & answer→Question 341 Mark
Write the expression for the equilibrium constant, Kc for each of the following reactions:
$\text{CH}_3\text{COOC}_2\text{H}_5\text{(aq)}+\text{H}_2\text{O(l)}\rightleftharpoons\text{CH}_3\text{COOH(aq)+}\text{C}_2\text{H}_5\text{OH(aq)}$
Answer$\text{K}_{\text{c}}=\frac{[\text{CH}_3\text{COOH(aq)]}[\text{C}_2\text{H}_5\text{OH(aq)}]}{[\text{CH}_3\text{COOC}_2\text{H}_5\text{(aq)}][\text{H}_2\text{O(l)}]}$
$=\frac{[\text{CH}_3\text{COOH(aq)]}[\text{C}_2\text{H}_5\text{OH(aq)}]}{[\text{CH}_3\text{COOC}_2\text{H}_5\text{(aq)}]}$
View full question & answer→Question 351 Mark
Which of the followings are Lewis acids? H2O, BF3, H+, and $\text{NH}_4^+$
AnswerBF3, H+ and $\text{NH}_4^+$ are Lewis acids because they can accept a lone pair of electrons.
View full question & answer→Question 361 Mark
Write the expression for the equilibrium constant, Kc for each of the following reactions:
$\text{2Cu(NO}_3)_2\rightleftharpoons\text{2CuO (s) + 4NO}_2\text{ (g) + O}_2\text{ (g)}$
Answer$\text{K}_{\text{c}}=\frac{[\text{CuO(g)]}^2[\text{NO}_2\text{(g)}]^4[\text{O}_2\text{(g)]}}{[\text{Cu(NO}_3)_2\text{}\text{(s)}]^2}=[\text{NO}_2\text{(g)}]^4[\text{O}_2\text{(g)}]$
View full question & answer→Question 371 Mark
Describe the effect of:
addition of CH3OH
on the equilibrium of the reaction:
$2\text{H}_2\text{ (g) + CO (g)}\rightleftharpoons\text{CH}_3\text{OH (g)}$
AnswerOn addition of CH3OH, the equilibrium will shift in the backward direction.
View full question & answer→Question 381 Mark
Describe the effect of:
removal of CO
on the equilibrium of the reaction:
$2\text{H}_2\text{ (g) + CO (g)}\rightleftharpoons\text{CH}_3\text{OH (g)}$
AnswerOn removing CO, the equilibrium will shift in the backward direction.
View full question & answer→Question 391 Mark
The equilibrium constant expression for a gas reaction is,
$\text{K}_{\text{c}}=\frac{[\text{NH}_3]^4[\text{O}_2]^5}{[\text{NO}]^4[\text{H}_2\text{O}]^6}$
Write the balanced chemical equation corresponding to this expression.
AnswerBalanced chemical equation for the reaction is 4
$4\text{NO (g) + 6H}_2\text{O (g)}\rightleftharpoons4\text{NH}_3\text{ (g) + 5O}_2\text{ (g)}$
View full question & answer→Question 401 Mark
Write the expression for the equilibrium constant, Kc for each of the following reactions:
$\text{2NOCl(g)}\rightleftharpoons\text{2NO (g) + Cl}_2\text{ (g)}$
Answer$\text{K}_{\text{c}}=\frac{[\text{NO(g)]}^2[\text{Cl}_2\text{(g)}]}{[\text{NOCl(g)}]^2}$
View full question & answer→Question 411 Mark
Write the expression for the equilibrium constant, Kc for each of the following reactions: $\text{Fe}^{3+}\text{(aq)}+3\text{OH}^-\text{(aq)}\rightleftharpoons\text{Fe(OH})_3\text{(S)}$
Answer$\text{K}_{\text{c}}=\frac{[\text{Fe(OH})_3\text{(S)]}}{[\text{Fe}^{3+}\text{(aq)}][\text{OH}^-\text{(aq)}]^3}$
$=\frac{1}{[\text{Fe}^{3+}\text{(aq)}][\text{OH}^-\text{(aq)}]^3}$
View full question & answer→Question 421 Mark
What is the effect of temperature on solubility product (Ksp)?
AnswerKsp increases with increase in temperature because solubility increases.
View full question & answer→Question 431 Mark
Classify the following as Lewis acid or Lewis base:
$\text{NH}_4^+\text{ and }\text{NH}_3$
Answer$\text{NH}^+_4$ Lewis acid, whereas NH3 is Lewis base.
View full question & answer→Question 441 Mark
What happens to ionic product of water if some acid is added to it?
AnswerIonic product will remain unchanged.
View full question & answer→Question 451 Mark
Under what conditions is a substance precipitated from its solution?
AnswerPrecipitation takes place, when ionic product exceeds the solubility product.
View full question & answer→Question 461 Mark
Write expression of Kp for the reaction:
$\text{N}_2\text{O(g)}\rightleftharpoons2\text{NO}_2(\text{g})$
Answer$\text{K}_{\text{p}}=\frac{(\text{P}_{\text{NO}_2})^2}{(\text{P}_{\text{N}_2\text{O}_4})}$
View full question & answer→Question 471 Mark
Why is solubility of AgI in NaI in less than that of pure water?
AnswerIt is due to common ion effect. I- will combine with Ag+ to from AgI, therefore solubility of AgI will decrease.
$\text{A}_2\text{B}\rightleftharpoons2\text{A}^++\text{B}^{2-}\\'\text{s}'\ \ \ \ \ \ \ \ \ \ \ \text{2s}\ \ \ \ \ \ \ \ '\text{s}'$
$\text{K}_{\text{sp}}=[\text{A}^+]^2[\text{B}^{2-}]$
$32\times10^{-9}=4\text{s}^3$
$32\times10^{-9}=4\text{s}^{3}$
$\text{s}^3=8\times10^{-9}$
$\text{s}=2\times10^{-3}\text{mol L}^{-1}$
$[\because3\sqrt{8}=2]\text{ and }(10^{-9})\frac{1}{3}=10^{-3}$
View full question & answer→Question 481 Mark
For Tribasic acid Ka1 > Ka2 > Ka3 what will happen to the acid strength of polyprotic acids if protons are lost?
AnswerAcid strength will decrease because Ka2, is less than Ka1 and K a3 is less than Ka2
View full question & answer→Question 491 Mark
Which of the following is weakest acid? $\text{HClO}_4,\text{HClO}_3,\text{HCl}_2,\text{HClO}$
AnswerHCl4O is weakest acid because Cl is in +1 oxidation state, i.e., lowest oxidation state.
View full question & answer→Question 501 Mark
Write the expression for the equilibrium constant (Kc) for the reaction:
$\text{CH}_3\text{COOC}_2\text{H}_5(\text{aq})+\text{H}_2\text{O(l)}\\\rightleftharpoons\text{CH}_3\text{COOH}(\text{aq})+\text{C}_2\text{H}_5\text{OH}(\text{aq})$
Answer$\text{K}_{\text{c}}=\frac{[\text{CH}_3\text{COOH}][\text{C}_2\text{H}_5\text{OH}]}{[\text{CH}_3\text{COOC}_2\text{H}_2\text{H}_5][\text{H}_2\text{O}]}$
View full question & answer→Question 511 Mark
Write the equilibrium constant expression for following reaction:
$2\text{NOCl}(\text{g})\rightleftharpoons2\text{NO(g)}+\text{Cl}_2(\text{g})$
Answer$\text{K}=\frac{[\text{NO}^2][\text{Cl}_2]}{[\text{NOCl}^2]}$
View full question & answer→Question 521 Mark
Why pH of our blood remains constant at 7.4 through we quite often eat spicy food?
AnswerBlood contains basic buffer which keep its pH constant.
View full question & answer→Question 531 Mark
Write Kp in terms of Kc for the following chemical reaction:
$2\text{SO}_2(\text{g})+\text{O}_2(\text{g})\rightleftharpoons2\text{SO}_3\text{(g)}$
Answer$\text{K}_{\text{p}}=\text{K}_{\text{c}}(\text{RT}^{\Delta\text{n}})$
$\Delta\text{n}=2-3=-1$
$\text{K}_{\text{c}}(\text{RT})^{-1}$
View full question & answer→Question 541 Mark
$\text{SO}_3^{2-}$ is Bronsted base or acid and why?
Answer$\text{SO}_3^{2-}$ is Bronsted base because it can accept H+.
View full question & answer→Question 551 Mark
What is the conjugate base of [Fe(H2O)6]3+?
Answer[Fe(H2O)5OH]2+ is conjugate base of [Fe(H2O)6]3+.
View full question & answer→Question 561 Mark
Which of the following is strongest Lewis acid?
$\text{CCl}_4,\text{AlCl}_3,\text{NCl}_3,\text{OCl}_2$
AnswerAlCl3 is strongest Lewis acid because its octet is not complete.
View full question & answer→Question 571 Mark
Fizz is observed when soda water bottle is opened. Why?
AnswerPressure is decreased, solubility of CO2 in water decreases, CO2 escapes from cold drink bottle.
View full question & answer→Question 581 Mark
Which of the following is strongest conjugate base?
$\text{CH}_3^-,\text{NH}^-_2,\text{OH}^-,\text{F}^-$
Answer$\text{CH}_4^-$ is strongest conjugate base because CH4 is weakest acid, i.e., cannot donate H+ easily.
View full question & answer→Question 591 Mark
Write expression of Kc for reaction:
$\text{N}_2(\text{g})+3\text{H}_2(\text{g})\rightleftharpoons2\text{NH}_3(\text{g})$
Give units of K.
Answer$\text{K}=\frac{[\text{NH}_3]^2}{[\text{N}_2][\text{H}_2]^3}$
$=\frac{(\text{mol L}^{-1})^2}{(\text{mol}^{-1})(\text{mol L}^{-1})^3}=\text{L}^2\text{mol}^{-2}$
View full question & answer→Question 601 Mark
How does common ion affect the solubility of electrolyte?
AnswerSolubility of electroyte decreases due to common ion effect.
View full question & answer→Question 611 Mark
Write the conjugate acid for the Bronsted base $\text{C}_6\text{H}_5\text{OH},\text{H}_2\text{O}$
Answer$\ \ \ \ \ \ \ \ \oplus{}\ \ \ \ \ \ \ \ \ \ \oplus{}\\\text{C}_6\text{H}_5\text{OH}_2,\text{H}_3\text{O}$
View full question & answer→Question 621 Mark
If Qc < Kc, in which direction reaction will proceed?
AnswerIf Qc < Kc, the reaction will proceed in the direction of products.
View full question & answer→Question 631 Mark
Which of the following is not Lewis base Ag+, H2O, CN-, NH3.
AnswerAg+, It is Lewis acid because it is positively charged and can accept electrons.
View full question & answer→Question 641 Mark
Why is Lewis concept more useful than Bronsted Lowry concept?
AnswerLewis concept includes some of compounds like BF3, BCl3, AlCl3 as acids which Bronsted Lowry concept does not.
View full question & answer→Question 651 Mark
Is it possible to get precipitate of Fe(OH)2 at pH = 2? Give reason.
AnswerNo, Because Fe(OH)3 will dissolve in strongly acidic medium.
View full question & answer→Question 661 Mark
Is it possible to get precipitate of Fe(OH)3 at pH = 2? Give reason.
AnswerNo, because Fe(OH)3 will dissolve in strongly acidic medium.
View full question & answer→