Find pH of solution when 100 ml of 0.1 N HCL is mixed with 100 ml of 0.1 M of NH4OH solution
Answers
Answer:
5.27
Explanation:
NH4OH + HCl =====> NH4Cl. So when 0.1-M NH4OH is neutralized by HCl, NH4Cl will be obtained.
Its concentration will be =0.1/2= 0.05-M.
Since it is a salt of a weak base (NH4OH) and a strong acid ( HCl), the solution will be acidic.
Its pH will be
pH= ½{pKw - pKb- logC} here
pKw= 14
pKb- for NH4OH= 4.7447
(since Kb=1.8 x 10^-5)
log C= log(0.05)=- 1.3010
So pH= ½{14–4.7447+1.3010) = 10.5563/2
= 5.2782 .
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Answer:
pH=10.96
Explanation:
The pH of an answer is a degree of hydrogen ion awareness, which in flip is a degree of its acidity. Pure water dissociates barely into same concentrations of hydrogen and hydroxyl (OH−) ions. For a impartial answer, [H+] is 10−7, or pH = 7.To calculate the pH of an aqueous answer you want to understand the awareness of the hydronium ion in moles according to liter (molarity). The pH is then calculated the usage of the expression: pH = - log [H3O+].
NaOH + HCl→ NaCl + H 2O
So, 1 mol NaOH reacts with 1 mol HCl
Moles of HCl in 9.9mL of 1.0M answer = 9.9/1000x1=0.0099mol HCL
Moles of NaOH in 100mL of 0.1M answer = 100/1000x0.1=0.01 mol NaOH
On blending the 0.0099 mol HCl may be neutralised and 0.01 - 0.0099 = 1x10^-4
mol NaOH dissolved in 109.9mL answer
Molarity of NaOH answer =1x10^-4/0.1099=9.099x10^-4M
Hence,
pOH = -log (9.099x10^-4)
pOH = 3.04
So,
pH = 14.00 - pOH
pH = 14.00 - 3.04
pH=10.96
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