Chapter 9: Q2P (page 208)

Neglecting activity coefficients, calculate the pHof $1.0 \times 10^{- 2} M KOH$

Short Answer

Expert verified

The pH of $1.0 \times 10^{- 2} M KOH$ is 12.00.

Step by step solution

Step: Definition of pH

pH is defined as a quantitative measure of acidity and basicity.Compounds having pH more than 7 is acidic in nature while pH when shown above than 7 is basic in nature. When pH comes 7 , compound is said to be neutral.

Step: Disassociation of HBr

$HBr$ is a strong acid and thus will completely disassociate. Thus, the concentration of $HBr$ is equal to the concentration of localid="1654776012313" $[HBr] = H^{+}$ .

Step: Calculating pH

$pOH = - \log (1.0 \times 10^{- 2}) = 2.00 pH = 14 - pOH = 14 - 2 = 12.00$

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Neglecting activity coefficients, calculate the pHof $1.0 \times 10^{- 2} M KOH$

Short Answer

Step by step solution

Step: Definition of pH

Step: Disassociation of HBr

Step: Calculating pH

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Neglecting activity coefficients, calculate the pHof 1.0×10-2MKOH

Short Answer

Step by step solution

Step: Definition of pH

Step: Disassociation of HBr

Step: Calculating pH

One App. One Place for Learning.

Most popular questions from this chapter

Recommended explanations on Chemistry Textbooks

Making Measurements

Kinetics

Organic Chemistry

Nuclear Chemistry

Inorganic Chemistry

Chemistry Branches

Study anywhere. Anytime. Across all devices.

Neglecting activity coefficients, calculate the pHof $1.0 \times 10^{- 2} M KOH$