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GaryK [48]
2 years ago
9

What volume of a 0.252 M hydroiodic acid solution is required to neutralize 18.0 mL of a 0.151 M barium hydroxide solution

Chemistry
1 answer:
zhenek [66]2 years ago
6 0

Answer: 10.8 M

Explanation:

M_{A}V_{A}=M_{B}V_{B}\\(0.252)V_{A}=(18.0)(0.151)\\V_{A}=\frac{(18.0)(0.151)}{(0.252)} \approx \boxed{10.8 \text{ M}}

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The pH of 0.10 M solution of an acid is 6. What is the acid dissociation constant of the acid?
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                         HA\rightleftharpoons H^++A^-

pH of the solution = 6

and we know that

pH=-log([H^+])

[H^+]=antilog(-pH)

[H^+]=antilog(-6)=10^{-6}M

As HA ionizes into its ions in 1 : 1 ratio, hence

[H^+]=[A^-]=10^{-6}M

As the reaction proceeds, the concentration of acid decreases as it ionizes into its ions, hence the decreases concentration of acid at equilibrium will be:

[HA]=[HA]-[H^+]

[HA]=0.1M-10^{-6}M

[HA]=0.09999M

Dissociation Constant of acid, K_a is given as:

K_a=\frac{[A^-][H^+]}{HA}

Putting values of [H^+],[A^-]\text{ and }[HA] in the above equation, we get

K_a=\frac{(10^{-6}M).(10^{-6}M)}{0.09999M}

K_a=1.0001\times 10^{-11}M

Rounding it of to one significant figure, we get

K_a=1.0\times 10^{-11}M\approx 10^{-11}M

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