Calculate the $p H$ of the resulting solution formed by mixing the following solutions.
$2 m L$ of $0.1 M H C l$ + $10 m L$ of $0.01 M S r (O H)_{2}$

Open in App

Solution

$m$ moles of $H^{+} = 0.2$
$m$ moles of $O H^{-} = 10 \times 0.01 \times 2 = 0.2$
Hence, the acid & base are completely neutralized and the salt $S r C l_{2}$ is formed.
$∴ p H = 7$ (neutral)

Suggest Corrections

Similar questions

p H

10 m L

0.2 M H C l

40 m L

0.1 M H_{2} S O_{4}

H_{2} S O_{4} .

50 mL of 0.1 M HCl and 50 mL of 2.0 M NaOH are mixed. The pH of the resulting solution is -

Consider $l o g (2) = 0.30$

50 m l

0.1 M H C l

49.9 m l

0.1 M N a O H

p H

60 m l

0.1 M H C l

40 m l

0.05 M H_{2} S O_{4}

p H

Join BYJU'S Learning Program