   Chapter 21, Problem 116IL

Chapter
Section
Textbook Problem

Sodium borohydride, NaBH4, reduces many metal ions to the metal.(a) Write a balanced equation for the reaction of NaBH4 with AgNO3 in water to give silver metal, H2 gas, boric acid, and sodium nitrate. (The chemistry of NaBH4 is described in Section 21.6.)(b) What mass of silver can be produced from 575 mL of 0.011 M AgNO3 and 13.0 g of NaBH4?

(a)

Interpretation Introduction

Interpretation:

To write the balanced equation for the reaction of NaBH4 with AgNO3 in water.

Concept introduction:

Reducing agent are the species that reduces another species and itself gets oxidized in a chemical reaction. A common example of reducing agent is sodium borohydride. The formula for sodium borohydride is NaBH4. It reacts with compounds having metal ions and reduces them to free metal.

A balanced chemical equation occurs when the number of atoms in reactant side is equal to the number of atoms in the product side.

Explanation

Sodium borohydride reacts with silver nitrate in the presence of water to give silver metal, hydrogen gas, boric acid and sodium nitrate. The equation is multiplied with stoichiometric coefficient to have equal number of atoms on both the reactant and product side.

Thus, the balanced equation for the reaction of NaBH4 with AgNO3 in water is,

2NaBH4(s)+2AgNO3(s

(b)

Interpretation Introduction

Interpretation:

The mass of silver produced in the reaction has to be stated.

Concept introduction:

Reducing agent are the species that reduces another species and itself gets oxidized in a chemical reaction. A common example of reducing agent is sodium borohydride. The formula for sodium borohydride is NaBH4. It reacts with compounds having metal ions and reduces them to free metal.

A balanced chemical equation occurs when the number of atoms in reactant side is equal to the number of atoms in the product side.

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