If it requires 37.5 mL of a 0.245 M HBr solution to neutralize 18.0 mL Mg (OH) 2, what is the concentration of the Mg (OH) 2 solution? 2 HBr + Mg (OH) 2 yields Mg (Br) 2 + 2 H2O

Question

Chemistry

Kyson

21 November, 09:03

If it requires 37.5 mL of a 0.245 M HBr solution to neutralize 18.0 mL Mg (OH) 2, what is the concentration of the Mg (OH) 2 solution? 2 HBr + Mg (OH) 2 yields Mg (Br) 2 + 2 H2O

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Answers (1)

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Misael Pollard · Answer 1

2 HBr + Mg (OH) 2 yields Mg (Br) 2 + 2 H2O

M1V1 = M2V2

(0.245 M) (37.5 mL) = (M2) (18.0 mL)

9.1875 = (M2) (18.0 mL)

9.1875 / (18.0 mL) = (M2) (18.0 mL) / (18.0 mL)

0.51041

this is not the complete answer as the mol to mol ratio must be considered!

For every 2 mols of HBr there is 1 mole of Mg (OH) 2; ratio = 2:1

0.51041 / 2 = 0.25520

M2 = 0.25520

0.25520 M of Mg (OH) 2 solution