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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

Question: Show by suitable net ionic equations that each of the following species can act as a Bronsted-Lowry acid: (a) \(HN{O_3}\) (b) \(PH_4^ + \) (c) \({H_2}S\) (d) \(C{H_3}C{H_2}COOH\) (e) \({H_2}PO_4^ - \) (f) \(H{S^ - }\)

The hydronium ion concentration in a sample of rainwater is found to be \(1.7 \times 1{0^{ - 6}}M\) times 25oC. What is the concentration of hydroxide ions in the rainwater?

What are amphiprotic species? Illustrate with suitable equations.

Explain why equilibrium calculations are not necessary to determine ionic concentrations in solutions of certain strong electrolytes such as. \(NaOH\;and\;HCl.\;\) Under what conditions are equilibrium calculations necessary as part of the determination of the concentrations of all ions of some other strong electrolytes in solution?

Identify and label the Brønsted-Lowry acid, its conjugate base, the Brønsted-Lowry base, and its conjugate acid in each of the following equations:

\({\rm{\;(a)\;NO}}_2^ - + {{\rm{H}}_2}{\rm{O}} \to {\rm{HN}}{{\rm{O}}_2} + {\rm{O}}{{\rm{H}}^ - }\).

\({\rm{\;(b)\;HBr}} + {{\rm{H}}_2}{\rm{O}} \to {{\rm{H}}_3}{{\rm{O}}^ + } + {\rm{B}}{{\rm{r}}^ - }\)

\({\rm{\;(c)\;H}}{{\rm{S}}^ - } + {{\rm{H}}_2}{\rm{O}} \to {{\rm{H}}_2}{\rm{S}} + {\rm{O}}{{\rm{H}}^ - }\)

\({\rm{\;(d)\;}}{{\rm{H}}_2}{\rm{PO}}_4^ - + {\rm{O}}{{\rm{H}}^ - } \to {\rm{HP}}{{\rm{O}}_4}^{2 - } + {{\rm{H}}_2}{\rm{O}}\)

\({\rm{\;(e)\;}}{{\rm{H}}_2}{\rm{PO}}_4^ - + {\rm{HCl}} \to {{\rm{H}}_3}{\rm{P}}{{\rm{O}}_4} + {\rm{C}}{{\rm{l}}^ - }\)

\({\rm{\;(f)\;}}{\left( {{\rm{Fe}}{{\left( {{{\rm{H}}_2}{\rm{O}}} \right)}_5}({\rm{OH}})} \right)^{2 + }} + {\left( {{\rm{Al}}{{\left( {{{\rm{H}}_2}{\rm{O}}} \right)}_6}} \right)^{3 + }} \to {\left( {{\rm{Fe}}{{\left( {{{\rm{H}}_2}{\rm{O}}} \right)}_6}} \right)^{3 + }} + {\left( {{\rm{Al}}{{\left( {{{\rm{H}}_2}{\rm{O}}} \right)}_5}({\rm{OH}})} \right)^{2 + }}\)

\({\rm{\;(g)\;C}}{{\rm{H}}_3}{\rm{OH}} + {{\rm{H}}^ - } \to {\rm{C}}{{\rm{H}}_3}{{\rm{O}}^ - } + {{\rm{H}}_2}\)
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