The pH of a 0.05 M solution of H 2 SO 4 in water is nearly

Question

The pH of a 0.05 M solution of H 2 SO 4 in water is nearly (A) 0.05 (B) 1 (C) -1 (D) 0

Tardigrade Admin · Accepted Answer

pH =- log 10 H + The concentration of H + ions is expressed in gram equivalent Molarity of H 2 SO 4=0.05 ∴ Normality =0.05 × 2=0.1 ∴ pH =- log 0.1 or pH =1

Q. The pH of a $0.05 M$ solution of $H_{2} S O_{4}$ in water is nearly

0.05

1

-1

0

$p H = - lo g_{10} H^{+}$

The concentration of $H^{+}$ ions is expressed in gram equivalent Molarity of $H_{2} S O_{4} = 0.05$

$∴$ Normality $= 0.05 \times 2 = 0.1$

$∴ p H = - lo g 0.1$ or $p H = 1$

Q. The pH of a 0.05M solution of H2​SO4​ in water is nearly

0.05

1

-1

0

pH=−log10​H+ The concentration of H+ ions is expressed in gram equivalent Molarity of H2​SO4​=0.05 ∴ Normality =0.05×2=0.1 ∴pH=−log0.1 or pH=1

Q. The pH of a $0.05 M$ solution of $H_{2} S O_{4}$ in water is nearly

$p H = - lo g_{10} H^{+}$

The concentration of $H^{+}$ ions is expressed in gram equivalent Molarity of $H_{2} S O_{4} = 0.05$

$∴$ Normality $= 0.05 \times 2 = 0.1$

$∴ p H = - lo g 0.1$ or $p H = 1$