Assuming complete ionization, the pH of 0.1 M, HCl is 1. The molarity of H2SO4 with the same pH is

Question

Assuming complete ionization, the pH of 0.1 M, HCl is 1. The molarity of H2SO4 with the same pH is (A) 0.1 (B) 0.2 (C) 0.05 (D) 2.0

Tardigrade Admin · Accepted Answer

pH of 0.1 HCl= 1 H2SO-4 leftharpoons H++HSO-4 HSO-4 leftharpoons H++SO2-4 ∴ H2SO4 ionises to give two H+ ions ∴ 0.05 M H2SO4 will give 0. 1 M H+ ion ∴ the molarity of H2SO4 = 0.05

Q. Assuming complete ionization, the pH of $0.1 M, H Cl$ is $1$ . The molarity of $H_{2} S O_{4}$ with the same pH is

0.1

0.2

0.05

2.0

$p H$ of $0.1 H Cl = 1$
$H_{2} S O_{4}^{-} ⇌ H^{+} + H S O_{4}^{-}$
$H S O_{4}^{-} ⇌ H^{+} + S O_{4}^{2 -}$
$∴ H_{2} S O_{4}$ ionises to give two $H^{+}$ ions
$∴ 0.05 M H_{2} S O_{4}$ will give $0.1 M H^{+}$ ion
$∴$ the molarity of $H_{2} S O_{4} = 0.05$

Q. Assuming complete ionization, the pH of 0.1M,HCl is 1. The molarity of H2​SO4​ with the same pH is

0.1

0.2

0.05

2.0

pH of 0.1HCl=1 H2​SO4−​⇌H++HSO4−​ HSO4−​⇌H++SO42−​ ∴H2​SO4​ ionises to give two H+ ions ∴0.05MH2​SO4​ will give 0.1MH+ ion ∴ the molarity of H2​SO4​=0.05

Q. Assuming complete ionization, the pH of $0.1 M, H Cl$ is $1$ . The molarity of $H_{2} S O_{4}$ with the same pH is

$p H$ of $0.1 H Cl = 1$
$H_{2} S O_{4}^{-} ⇌ H^{+} + H S O_{4}^{-}$
$H S O_{4}^{-} ⇌ H^{+} + S O_{4}^{2 -}$
$∴ H_{2} S O_{4}$ ionises to give two $H^{+}$ ions
$∴ 0.05 M H_{2} S O_{4}$ will give $0.1 M H^{+}$ ion
$∴$ the molarity of $H_{2} S O_{4} = 0.05$