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Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

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BuyFindarrow_forward

Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
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. Of the following conditions, which indicate a basic solution?

a. pOH = 12.53

b. pH=3.64

c. pOH< [ H + ]

d. [ OH ] > 1.0 × 10 7 M

Interpretation Introduction

Interpretation:

Among the given conditions, the condition which represents a basic solution should be identified.

pOH = 12.53

pH=3.64

pOH<[H+]

[OH]>1.0×107 M.

Concept Introduction:

Water is an amphoteric in nature implies it can act as an acid as well as base.

Ionization of water is given as:

H2O(l)+H2O(l)H+(aq)+OH(aq)

Here, one water molecule is act as an acid by accepting proton and another molecule of water act as a base by donating proton.

At 25°C, the actual concentrations of the products are:

[H+][OH]=1×1014

To express the small number, p scale is used, which implies to take the log of a number. Since, the concentration of [H+] in aqueous solution is small, by using the p scale in the form of pH scale, it is better way to represent acidity of solution.

Thus, pH = -log [H+]

Similarly, the relation between pOH and [OH] is given by:

pOH=-log [OH]

The solution is basic when its pH is equal to greater than 7.

Explanation

Reason for correct option:

[OH]>1.0×107 M

pOH<-log (1.0×107<

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