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Chapter 16: Problem 68

Specify which of these salts will undergo hydrol\(\begin{array}{llll}\text { ysis: } \mathrm{KF}, & \mathrm{NaNO}_{3}, & \mathrm{NH}_{4} \mathrm{NO}_{2}, & \mathrm{MgSO}_{4}, & \mathrm{KCN},\end{array}\) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COONa}, \mathrm{RbI}, \mathrm{Na}_{2} \mathrm{CO}_{3}, \mathrm{CaCl}_{2}, \mathrm{HCOOK}\).

Short Answer

Expert verified
The salts that will undergo hydrolysis are KF, NH4NO2, MgSO4, KCN, Na2CO3, and HCOOK.

Step by step solution

01

Determine the ions

The first step to determine whether these salts will undergo hydrolysis or not is to look at their ions. A salt is made up of a cation (positive ion) and an anion (negative ion). The salts have the following cations and anions: KF has K+ and F-, NaNO3 has Na+ and NO3-, NH4NO2 has NH4+ and NO2-, MgSO4 has Mg2+ and SO42-, KCN has K+ and CN-, C6H5COONa has C6H5COO- and Na+, RbI has Rb+ and I-, Na2CO3 has Na+ and CO32-, CaCl2 has Ca2+ and 2Cl-, and HCOOK has HCOO- and K+.
02

Determine the ability to undergo hydrolysis

Hydrolysis occurs when ions from the salt react with water. Salts of neutral pH won't undergo hydrolysis, meaning if the anion and cation both come from strong bases and strong acids respectively, the salt will not undergo hydrolysis. Salts with cations of weak bases or anions from weak acids will undergo hydrolysis. Through this approach, the salts that would undergo hydrolysis would be: KF, NH4NO2, MgSO4, KCN, Na2CO3, and HCOOK.
03

Summarize Findings

The salts that would undergo hydrolysis are: KF (due to F-, which comes from weak acid HF), NH4NO2 (due to NH4+, which comes from weak base NH3), MgSO4 (due to Mg2+, which comes from weak base Mg(OH)2), KCN (due to CN-, which comes from weak acid HCN), Na2CO3 (due to CO32-, which comes from weak acid H2CO3), and HCOOK (due to HCOO-, which comes from weak acid HCOOH).

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Most popular questions from this chapter

Write the equation relating \(K_{\mathrm{a}}\) for a weak acid and \(K_{\mathrm{b}}\) for its conjugate base. Use \(\mathrm{NH}_{3}\) and its conjugate acid \(\mathrm{NH}_{4}^{+}\) to derive the relationship between \(K_{\mathrm{a}}\) and \(K_{\mathrm{b}}\).

Which of the following is the stronger acid: \(\begin{array}{llll}\mathrm{CH}_{2} \mathrm{ClCOOH} & \text { or } \mathrm{CHCl}_{2} \mathrm{COOH} ? & \text { Explain your }\end{array}\) choice.

Give the conjugate base of each of these acids: (a) \(\mathrm{CH}_{2} \mathrm{ClCOOH},\) (b) \(\mathrm{HIO}_{4}\) (c) \(\mathrm{H}_{3} \mathrm{PO}_{4},\) (d) \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) (e) \(\mathrm{HPO}_{4}^{2-},\) (f) \(\mathrm{H}_{2} \mathrm{SO}_{4},(\mathrm{~g}) \mathrm{HSO}_{4}^{-}\) (h) \(\mathrm{HCOOH}\) (i) \(\mathrm{HSO}_{3}^{-},(\mathrm{j}) \mathrm{NH}_{4}^{+},(\mathrm{k}) \mathrm{H}_{2} \mathrm{~S},\) (l) \(\mathrm{HS}^{-},(\mathrm{m}) \mathrm{HClO}\).

Most of the hydrides of Group \(1 \mathrm{~A}\) and Group \(2 \mathrm{~A}\) metals are ionic (the exceptions are \(\mathrm{BeH}_{2}\) and \(\mathrm{MgH}_{2}\), which are covalent compounds). (a) Describe the reaction between the hydride ion \(\left(\mathrm{H}^{-}\right)\) and water in terms of a Bronsted acid-base reaction. (b) The same reaction can also be classified as a redox reaction. Identify the oxidizing and reducing agents.

Which of the following solutions has the highest \(\mathrm{pH} ?\) (a) \(0.40 \mathrm{M} \mathrm{HCOOH},\) (b) \(0.40 \mathrm{M} \mathrm{HClO}_{4}\) (c) \(0.40 \mathrm{M} \mathrm{CH}_{3} \mathrm{COOH}\).
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