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`        What is the resultant pH of a solution when 20ml of 0.1N NaOH is mixed with 20ml of 0.05M Ca(OH) 2 at 25C?`
9 months ago

```							when 20ml of 0.1N NaOH is mixed with 20ml of 0.05M Ca(OH)2 at 25CEquivalent weight of NaOH = molecular weight of NaOH because its acidity is oneNORMALITY of NaOH = MOLARITY of NaOH =.1Milli mole of NaOH=molarity x volume = 20x.1 = 2NaOH——->Na+ + OH-2 milli mole of NaOH produce 2 milli mole of OH-Milli mole of Ca(OH)2=molarity x volume = 20x.05 = 1Ca(OH)2———→Ca+2 + 2OH-1 milli mole of Ca(OH)2 produce 2 milli mole of OH-Total milli mole of OH- = 1+2 = 3Total volume of solution(ml)=20+20=40mlOH- CONCENTRATION =Milli mole of OH-/Total volume of solution(ml)=3/40MpOH=-Log[OH-] = -log3/40 = log40-log3 =1.6020 -.4771 = 1.1249pH=14–1.1249=12.8751
```
9 months ago
```							@saood u idiot u have copied the answer from quora.. if u dont have the knowledge then dont answer.. or else i will complain against you idiot
```
9 months ago
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