Chemistry, asked by mithelesh001, 2 months ago


Calculate the pH of the solution formed by mixing 400 mL of 1 M HCl with 100 mL of 4.5 M NaOH.​

Answers

Answered by santwanamohanty3
0

Explanation:

Solution:- (B) 12

As we know that,

Molarity of a solution =

volume of solution

(in L)

no. of moles of solute

Given:-

Molarity of HCl solution =0.1M

Volume of HCl solution =40mL=0.04L

Therefore,

No. of moles of HCl=0.04×0.1=0.004 mol

Again,

Molarity of NaOH solution =0.45M

Volume of NaOH solution =10mL=0.01L

Therefore,

No. of moles of NaOH=0.01×0.45=0.0045 mol

Now, for the reaction-

NaOH+HCl⟶NaCl+H

2

O

NaOH is in excess.

Therefore,

Excess amount of NaOH=0.0045−0.004=0.0005 mol

Total volume =0.04+0.01=0.05L

Now,

[OH

]=

0.05

0.0005

=0.01M=10

−2

M

Therefore,

pOH=−log[OH

]

⇒pOH=−log(10

−2

)=2

Now as we know that,

pH+pOH=14

Therefore,

pH=14−pOH=14−2=12

Hence the pH of the solution is

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