Question

In a basic buffer, 0.0025 moles of nh4cl and 0.15 moles of nh4oh are present. The ph of the solution having pkb value of 4.74 will be

Answer 1

Explanation:

Calculate the pH of a buffer solution containing 0.2 mole of NH4Cl and 0.1 mole of ... According to Henderson – Hasselbalch equation: pOH = pKb + log ([salt]/ [base]) ... Chemistry. ·

Answer 2

The pH of the solution is 11.04

Explanation:

The chemical equation for the reaction of ammonium hydroxide with HCl follows:

$NH_4OH+HCl\rightarrow NH_4Cl+H_2O$

To calculate the pOH of basic buffer, we use the equation given by Henderson Hasselbalch:

$pOH=pK_b+\log(\frac{[salt]}{[base]})$

$pOH=pK_b+\log(\frac{[NH_4Cl]}{[NH_4OH]})$

We are given:

$pK_b$ = negative logarithm of base dissociation constant of ammonium hydroxide = 4.74

$[NH_4Cl]=\frac{0.0025}{V}$

$[NH_4OH]=\frac{0.15}{V}$

pOH = ?

Putting values in above equation, we get:

$pOH=4.74+\log(\frac{0.0025/V}{0.15/V})\\\\pOH=2.96$

To calculate pH of the solution, we use the equation:

$pH+pOH=14\\\\pH=14-2.96=11.04$

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