Question

The molar concentration of h+ ion when 0.1 m of 200ml hcl is mixed with 0.05 m of 300ml h2so4 solution is

Answer 1

0.1m is the molar concentration of the H+ ions

Explanation:

Given,

0.1 m of 200ml Hcl is diluted with 0.05m of 300 ml H2SO4

As we know,

HCL → $H^{+}$ + $Cl^{-}$

so,

No. of HCl moles in 0.1 M solution

0.01 M = Moles of HCl/0.2L

∵ HCl moles = 0.02

Since 1 HCl mole offers 1 mol of $H^{+}$ ions, 0.02 moles will offer 0.02 $H^{+}$ ions mol.

In $H_{2}SO_{4}$,

$H_{2}SO_{4}$ → $2H_{+} + SO_{4} ^{-}$

so,

No. of moles in 0.5 m solution

0.05 M = Moles of  $H_{2}SO_{4}$/0.3l                   (300ml/1000ml = 0.3 l)

$H_{2}SO_{4}$ Moles = 0.015 mol

Since 1  $H_{2}SO_{4}$ mole offers 2 mol of $H^{+}$ ions, 0.015 moles will offer 0.03 $H^{+}$ ions mol.

Thus, after diluting the solutions together, the molar concentration of $H^{+}$ ions:

M = moles of both the chemicals/amount of solution

= (0.02 + 0.03)/0.5                            (300 + 200/1000 = 0.5)

= 0.1 M

Learn more: Molarity

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