The concentration of `H^(+)` in a solution containing 0.2 mol of dichloroacetic acid `(Ka=5 times 10^(-2))` and 0.1 mol of sodium dichloroacetate in 1L of the solution is
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A buffer solution contains 0.1 M of acetic acid and 0.1 M of sodium acetate. What will be its pH ? ( pK_(a) of acetic acid is 4.75)
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Ethyl acetate is formed by the reaction between ethanol and acetic acid and equilibrium is represented as: 'CH_3 COOH_( )+C_2 H_5 OH_(l) hArr CH_3 COOC_2 H_5_(l)+H_2 O_(l)' i) Write the concentration ratio (reaction quotient), 'Q_c', for this reaction (note: water is not in excess and is not a solvent in this reaction) ii) At '293 K', if one starts with '1.00' mol of acetic acid and '0.18 mol' of ethanol, there is '0.171' mol of ethyl acetate in the final equilibrium mixture. Calculate the equilibrium constant. iii) Starting with '0.5' mol of ethanol and '1.0' mol of acetic acid and maintaining it at 293 ' K, '0.214' mol of ethyl acetate is found after sometime. Has equilibrium been reached?
The ratio of the pH of solution (I) containing 1 mol of CH_(3)COONa and 1 mol of HCl in 1L, and solution (II) containing 1 mol of CH_(3)COONa and 1 mol of CH_(3)COOH in 1L is
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BRILLIANT PUBLICATION-CHEMICAL AND IONIC EQUILIBRIUM-Level - III (Linked Comprehension Type Questions)
