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Chapter 4: Q4.29P (page 179)

Complete the following precipitation reactions with balanced molecular, total ionic, and net ionic equations:

(a)Hg2(NO3)2(aq)+KI(aq)鈫�(b)FeSO4(aq)+Sr(OH)2(aq)鈫�

Short Answer

Expert verified

Precipitation of ions depends upon the charge of ions present in a given solution.

Step by step solution

01

Write the equation of  Hg2(NO3)2and KI

The molecular reaction is:

Hg2(NO3)2(aq)+KI(aq)鈫�Hg2I2(s)+2KNO3(aq)

The total ionic equation is:

2Hg2+(aq)+2NO3-(aq)+2K+(aq)+2I-鈫�2K+(aq)+2NO3-(aq)+Hg2l2(s)

The net ionic equation is:

2Hg2+(aq)+2I-(aq)鈫�Hg2l2(s)

02

Write the equation of FeSO4(aq)  and Sr (OH)2

The molecular reaction is:

FeSO4(aq)+Sr(OH)2(aq)鈫�Fe(OH)2(s)+SrSO4(s)

The total ionic equation is:

Fe+2(aq)+SO4(aq)+Sr+2(aq)+2OH-(aq)鈫�Fe(OH)2(s)+SrSO4(s)

The net ionic equation is:

Fe+2(aq)+SO4(aq)+Sr+2(aq)+2OH-(aq)鈫�Fe(OH)2(s)+SrSO4(s)

Since this reaction does not have any spectator ion, hence both ionic and net ionic reaction is the same

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Most popular questions from this chapter

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

aCas+H2Ol鈫�CaOH2aq+H2g

bNaNO3s鈫�NaNO2s+O2g

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Iron reacts rapidly with chlorine gas to form a reddish brown, ionic compound (A), which contains iron in the higher of its two common oxidation states. Strong heating decomposes compound A to compound B, another ionic compound, which contains iron in the lower of its two oxidation states. When compound A is formed by the reaction of 50.6 g of Fe and 83.8 g of Cl2 and then heated, how much compound B forms?

Predict the product(s) and write a balanced equation for each of the following redox reactions:

(a) Pentane (C5H12) + Oxygen 鈫�

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(e) Write a balanced net ionic equation for (d).

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