Q2. Calculate the pH of a 6.73 x 10 M H3PO4 (phosphoric acid) solution. Molar mass H3PO4=97.994 Density H3PO4= 1.88 ml →-106 [ 20.19 × 10 -47 = -109(2014) +410916 ↓ pH = -log[H¹] Нуроч эзна трой mol PH=-luy [Ht?" CHP->
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![Q2. Calculate the pH of a 6.73 x 10 M H3PO4 (phosphoric acid) solution.
pH = -log[H¹]
Нуроч -3 зн+
V
Molar mass H3PO4= 97.994
mol
Density H3PO4 = 1.88
трой
ml
3x 6.73x10-4 = 20.19 x 10-4 m²
PH=-loy CHT? -> -10% (20.19 × 10 -47 = -109(2014)+-4104 10
↓
Pl+=2.69
G-1.30574
Q3. Calculate the [H] (concentration of the H¹) of a HCl solution when the pH = 2.88
**Hint to solve Q3: antilog
pH = -log[H]
CH+] = arriles (PH)
o`pl
i
10-2.88
g
mol
Molar mass HC1= 36.458.
↓
1.318 × 10 ²1x10
(1.32)
Density HCl = 1.18 E
ml](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F21c9e2c1-3922-4190-983a-755fc6e01f0b%2F7dc38796-75b2-488d-813e-5bff65432b18%2F2zlxbbf_processed.jpeg&w=3840&q=75)
The question is based on the concept of pH of the solution. It is defined as a negative logarithm of hydrogen ion concentration present in a solution.
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