# what is the ph of the resulting solution when equal volumes of 0.1

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## What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed?

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Question

## What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed?

**A**

## 7.0

**B**

## 1.04

**C**

## 12.65

**D**

## 2.0

Hard Open in App Solution Verified by Toppr

Correct option is C)

Hint: More concentrated the basic solution more will be its pH.Formula: pOH=−log [OH − ]

Step:1 To find mole of OH

−

ions formed after mixing both solutions.

When equal volumes of 0.1MNaOH and 0.01MHCl are mixed, as NaOH concentration is more that is why hydroxide ions will be in excess so, the hydroxide ion concentration is

OH − = 2 0.1−0.01 =0.045M

Step:2 To find pH of solution after mixing.

On substituting above value in formula,

pOH=−log [OH − ]

The pOH of the solution is pOH=−log [OH

− ]=−log 0.045=1.35

The pH of the solution is pH=14−pOH=14−1.35=12.65

Final answer: Option C

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## What is the pH of the resulting solution when equal volumes of 0.1 M N aOH and 0.01 M HCl are mixed?A. 1.04B. 7.0C. 12.65D. 2.0

What is the pH of the resulting solution when equal volumes of 0.1 M N aOH and 0.01 M HCl are mixed?A. 1.04B. 7.0C. 12.65D. 2.0

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What is the pH of the resulting solution when equal volumes of 0.1 M N aOH and 0.01 M HCl are mixed?A. 1.04B. 7.0C. 12.65D. 2.0

Question What is the p H

of the resulting solution when equal volumes of

0.1 M N a O H and 0.01 M H C l are mixed? A 7.0 B 1.04 C 12.65 D 2.0 Open in App Solution

The correct option is **C**

12.65 N 1 V 1 − N 2 V 2 =

equivalents of unreacted hydroxyl ions.

0.1 × 1 − 0.01 × 1 = [ O H − ] [ O H − ] = N R = 0.09 2 = 0.045 N p O H = − log ( 0.045 ) = 1.35 ∴ p H = 14 − p O H = 14 − 1.35 = 12.65 Suggest Corrections 14

SIMILAR QUESTIONS

**Q.**

Equal volumes of 0.1 M HCl and 0.1 M NaOH are mixed. The concentration of the resulting solution will be

**Q.**When equal volumes of pH=4 and pH=6 are mixed together then the pH of the resulting solution will be: [log 5=0.7]

**Q.**The pH pf a solution is 10 and that of another is 12. When equal volumes of these two are mixed, the pH of the resulting solution is

**Q.**What is the resultant

p H

of the solution if equal volumes of two solutions with

p H = 5 and p H = 9 are mixed at 25 o C ?

## What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed?

N(1)V(1)-N(2)V(2)=NV 0.1xx1-0.01xx1=Nxx2 [OH^(-)]=N(R)=(0.09)/(2)=0.045 N pOH= -log (0.045) =1.35 :. pH=14- pOH=14-1.35=12.65 :. S=10^(-3) M

Home > English > Class 11 > Chemistry > Chapter > Ionic Equilibium >

What is the pH of the resultin...

What is the pH pH

of the resulting solution when equal volumes of

0.1MNaOH 0.1MNaOH and 0.01MHCl 0.01MHCl are mixed?

Updated On: 27-06-2022

00 : 30

UPLOAD PHOTO AND GET THE ANSWER NOW!

Text Solution Open Answer in App A 7.0 7.0 B 1.04 1.04 C 12.65 12.65 D 2.0 2.0 Answer

The correct Answer is C

Solution N 1 V 1 − N 2 V 2 =NV N1V1-N2V2=NV 0.1×1−0.01×1=N×2 0.1×1-0.01×1=N×2 [O H − ]= N R = 0.09 2 =0.045N

[OH-]=NR=0.092=0.045N

pOH=−log(0.045)=1.35

pOH=-log(0.045)=1.35

∴pH=14−pOH=14−1.35=12.65

∴pH=14-pOH=14-1.35=12.65

∴S= 10 −3 M ∴S=10-3M

Answer

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