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Chapter 14: Q14.3-52 E (page 831)

Which of the following will increase the percentage of HF that is converted to the fluoride ion in water?

(a) Addition of \(NaOH\)

(b) Addition of \(HCl\)

(c) Addition of \(NaF\)

Short Answer

Expert verified

The addition of \({\rm{NaOH}}\) will increase the percentage of \({\rm{HF}}{\rm{.}}\) The reaction that forms based on the question asked is \(HF(aq) \to {H^ + }(aq) + {F^ - }(aq).\)

Step by step solution

01

Le Chatelier Principle

  • The Le Chatelier principle says that when a system is put out of balance by a change of any kind, the system will react in a way that minimizes the same change and return balance to the system.
  • So, to increase the number of products (as is required here), we need to either increase the concentrations of the reactants or decrease the concentrations of the products.
02

Explanation

  • (a) The addition of \({\rm{NaOH}}\)will increase the percentage of \({\rm{HF}}\)that is convertedto \({{\rm{F}}^ - }.\)\({\rm{O}}{{\rm{H}}^ - }\)\({\rm{O}}{{\rm{H}}^ - }\) ions react with the \({{\rm{H}}^ + }\)ions and lower the concentration of \({{\rm{H}}^ + }\)ions in the solution. Therefore, adding \({\rm{NaOH}}\)woulddecrease the concentration of the products and thus "push" the reaction equilibrium towards the products.
  • (b) The addition of \(HCl\) will not increase, but decrease the percentage of \(HF\) converted to \({F^ - }.\) The \({H^ + }\) ions from the \(HCl\) increases the concentration of the products and hence, it will "push" the reaction equilibrium towards the reactants.
  • (c) The addition of \(NaF\) will not increase, but decrease the percentage of \(HF\) converted to \({F^ - }\). The \({F^ - }\) ions from the \(NaF\) would increase the concentration of the products and "push" the equilibrium towards the reactants.
  • Hence, option (a) is the right answer.

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Most popular questions from this chapter

Are the concentrations of hydronium ion and hydroxide ion in a solution of an acid or a base in water directly proportional or inversely proportional? Explain your answer.

Determine \({K_a}\)for hydrogen sulfate ion, \(HS{O_4}^ - .\)In a \(0.10 - M\)solution the acid is \(29\% \)ionized.

What is the effect on the concentration of acetic acid, hydronium ion, and acetate ion when the following are added to an acidic buffer solution of equal concentrations of acetic acid and sodium acetate:

(a)\(HCl\)

(b)\(KC{H_3}C{O_2}\)

(c)\(NaCl\)

(d)\(KOH\)

(e)\(C{H_3}C{O_2}H\)

Rank the compounds in each of the following groups in order of increasing acidity or basicity, as indicated, and explain the order you assign.

  1. \(acidity: HCl, HBr, HI\)
  2. \(basicity:\;{H_2}O,O{H^ - },{H^ - },C{l^ - }\)
  3. \(basicity:\;Mg{(OH)_2},Si{(OH)_4},Cl{O_3}(OH)\)(Hint: Formula could also be written as \(HCl{O_4}\))
  4. \(acidity:\;HF,{H_2}O,N{H_3},C{H_4}\)

From the equilibrium concentrations given, calculate \({K_a}\)for each of the weak acids and \({K_b}\)for each of the weak bases.

\(\begin{aligned}(a)N{H_3}:\left( {O{H^ - }} \right) = 3.1 \times 1{0^{ - 3}}M\left( {NH_4^ + } \right) = 3.1 \times 1{0^{ - 3}}M;\left( {N{H_3}} \right) = 0.533M;\\(b)HN{O_2}:\left( {{H_3}{O^ + }} \right) = 0.011M;\left( {NO_2^ - } \right) = 0.0438M;\left( {HN{O_2}} \right) = 1.07M;\\(c){\left( {C{H_3}} \right)_3}\;N:\left( {{{\left( {C{H_3}} \right)}_3}\;N} \right) = 0.25M;\left( {{{\left( {C{H_3}} \right)}_3}N{H^ + }} \right) = 4.3 \times 1{0^{ - 3}}M;\left( {O{H^ - }} \right) = 4.3 \times 1{0^{ - 3}}M;\\(d)N{H_4} + :\left( {N{H_4} + } \right) = 0.100M;\left( {N{H_3}} \right) = 7.5 \times 1{0^{ - 6}}M;\left( {{H_3}{O^ + }} \right) = 7.5 \times 1{0^{ - 6}}M\end{aligned}\)

\(\begin{aligned}\left( {N{H_3}} \right) = 7.5 \times 1{0^{ - 6}}M\\\left( {{H_3}{O^ + }} \right) = 7.5 \times 1{0^{ - 6}}M\end{aligned}\)
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