Q2. Calculate the pH of a 6.73 x 10 M H3PO4 (phosphoric acid) solution. Molar mass H3PO4 = 97.994 pH = -log[H¹] Poy-3H+ трой mol PH=-lug CHT? Density H3PO4 = 1.88 -105 [ 20.19 × 10 -47=-=-109(20.145+4109 | ml
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![Q2. Calculate the pH of a 6.73 x 10 M H3PO4 (phosphoric acid) solution.
Molar mass H3PO4= 97.994
pH = -log[H]
H3PO4 - 3H+
трой
3x 6.73x10 = 20.19 x 10"
Pl+=(2.69
Q3. Calculate the [H] (concentration of the H*) of a HCl solution when the pH = 2.88
**Hint to solve Q3: antilog
Density H3PO4= 1.88
mol
ml
PH=-loy CHT] => -105 [ 20114 × 10 -4 7 = -109(2014) +-410916
↓
0-4m²
G-1.30574
pH = -log[H]
CH*]=artilag (pH)
-
10-PH
10-288
↓
Molar mass HC1=36.458
1.318x1013x10-³ m
mol
Density HC1=1.18 B
ml](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F21c9e2c1-3922-4190-983a-755fc6e01f0b%2F4ddc8b50-225e-40a4-9ddc-3359c9020683%2Fjq68soo_processed.jpeg&w=3840&q=75)
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