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Chapter 4: Q4.50 (page 180)

Question: Zinc hydroxide is insoluble in water but dissolves when a nitric acid solution is added. Why? Write balanced total ionic and net ionic equations, showing nitric acid as it actually exists in water and the reaction as a proton-transfer process.

Short Answer

Expert verified

Answer

Zinc hydroxide is insoluble in water but dissolves when a nitric acid solution is added because it is an acid-base reaction and nitrate ions readily displaceOH ions from zinc hydroxide.

Step by step solution

01

Determine different types of equations to represent aqueous ionic reactions

The molecular equation reveals the least about the species in solution and is actually somewhat misleading because it shows all the reactants and products as if they were intact undissociated compounds.

The total ionic equation is a much more accurate representation of the reaction because it shows all the soluble ionic substances dissociated into ions.

The net ionic equation is the most useful because it omits the spectator ions and shows the actual chemical change taking place.

02

Write the net ionic equation of the reaction between zinc hydroxide and nitric acid

Balanced molecular reaction:

Zn(OH)2(s)+2HNO3(aq)→Zn(NO3)2(aq)+2H2O(l)

The total ionic equation:

Zn(OH)2(s)+2H+(aq)+2NO3-(aq)→Zn2+(aq)+2NO3-(aq)+2H2O(l)

The net ionic equation:

Zn(OH)2(s)+2H+(aq)→Zn2+(aq)+2H2O(l)

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Most popular questions from this chapter

In the process of pickling, rust is removed from newly produced steel by washing the steel in hydrochloric acid:

(1)6HCl(aq)+Fe2O3(s)→2FeCl3(aq)+3H2O(l)

During the process, some iron is lost as well:

(2)2HCl(aq)+Fe(s)→FeCl2(aq)+H2(g)

(a) Which reaction, if either, is a redox process? (b) If reaction 2 did not occur and all the HCl were used, how many grams of Fe2O3 could be removed and FeCl3 produced in a 2.50x103-L bath of 3.00 MHCl? (c) If reaction 1 did not occur and all the HCl were used, how many grams of Fe could be lost and FeCl2 produced in a 2.50x103-L bath of 3.00 MHCl? (d) If 0.280 g of Fe is lost per gram of Fe2O3 removed, what is the mass ratio of FeCl2to FeCl3?

Use the oxidation number method to balance the following equations by placing coefficients in the blanks. Identify the reducing and oxidizing agents:

(a)_KOH(aq)+_H2O2(aq)+_Cr(OH)3(s)→_K2CrO4(aq)+_H2O(l)(b)_MnO4−(aq)+_ClO2−(aq)+_H2O(l)→_MnO2(s)+_ClO4−(aq)+OH−(aq)(c)_KMnO4(aq)+_Na2SO3(aq)+_H2O(l)→_MnO2(s)+_Na2SO4(aq)+_KOH(aq)(d)_CrO42−(aq)+_HSnO2−(aq)+_H2O(l)→_CrO2−(aq)+_HSnO3−(aq)+OH−(aq)(e)_KMnO4(aq)+_NaNO2(aq)+_H2O(l)→_MnO2(s)+_NaNO3(aq)+_KOH(aq)(f)_I−(aq)+_O2(g)+_H2O(l)→_I2(s)+_OH−(aq)

Explain why an oxidizing agent undergoes reduction.

In a titration of HNO3, you add a few drops of phenolphthalein indicator to 50.00 mL of acid in a flask. You quickly add 20.00 mL of 0.0502 MNaOH but overshoot the end point, and the solution turns deep pink. Instead of starting over, you add 30.00 mL of the acid, and the solution turns colorless. Then, it takes 3.22 mL of the NaOH to reach the end point. (a) What is the concentration of the HNO3solution? (b) How many moles of NaOH were in excess after the first addition?

Balance each of the following redox reactions and classify it as a combination, decomposition, or displacement reaction:

(a)Sb(s)+Cl2(g)→SbCl3(s)

(b)AsH3(g)→As(s)+H2(g)

(c)Zn(s)+Fe(NO3)2(aq)→Zn(NO3)2(aq)+Fe(s)
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