(Unionized, weak acid and common ion effect)
$HA + NaOH \to NaA + {H_2}O$
$NaA \to N{a^ + } + {A^ - }$ (ionized)
${K_a} = \frac{{[{H^ + }][{A^ - }]}}{{[HA]}}$
Given, $pH = 6,\,[{H^ + }] = 1 \times {10^{ - 6}}$
$[{H^ + }] = \frac{{{K_a}[Acid]}}{{[Salt]}}$
$\frac{{[Salt]}}{{[Acid]}} = \frac{{{K_a}}}{{[{H^ + }]}} = \frac{{{{10}^{ - 5}}}}{{{{10}^{ - 6}}}} = 10:1$
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$C(g) + 4H(g) \to C{H_4}(g),\,\Delta H = - {x_1}\,k\,cal$
$C{H_4}(g) \to C{H_3}(g) + H(g),\,\Delta H = + y\,k\,cal$
The bond energy of $C - H$ bond is
$\sigma \,\,1{s^2}\,\,{\sigma ^*}\,\,1{s^2}\,\sigma \,\,2{s^2}\,{\sigma ^*}\,2{s^2}\,\,\sigma \,2p_x^2\,\left\{ {{}_{\pi \,2p_z^2}^{\pi \,2p_y^2}} \right.$
Its bond order is