Answer:
0.08
Step-by-step explanation:
First, we begin by writing the balanced equation for the reaction. This is illustrated below:
2HNO3 + Sr(OH)2 → Sr(NO3)2 + 2H2O
From the balanced equation above,
The mole ratio of the acid (nA) = 2
The mole ratio of the base (nB) = 1
Next, the data obtained from the. This includes the following:
Volume of acid (Va) = 17.8 mL
Volume of base (Vb) = 24.7 mL
Molarity of base (Mb) = 0.299 M
Molarity of acid (Ma) =..?
pH =..?
Next, we shall determine the molarity of the acid. This can be obtained as follow:
MaVa/MbVb = nA/nB
Ma x 17.8/0.299 x 24.7 = 2/1
Cross multiply to express in linear form
Ma x 17.8 = 0.299 x 24.7 x 2
Divide both side by 17.8
Ma = (0.299 x 24.7 x 2) /17.8
Ma = 0.830M.
Therefore, the molarity of the acid, HNO3 is 0.830M
Finally, we can obtain the pH of the acid as follow:
We shall obtain the concentration of the hydrogen ion, [H+]. This is illustrated below:
HNO3 —> H+ + NO3-
From the balanced equation above,
1 mole of HNO3 produced 1 mole of H+.
Therefore, 0.830M HNO3 will also produce 0.830M H+.
Therefore, the concentration of the hydrogen ion, [H+] is 0.830M
pH = –Log [H+]
[H+] = 0.830M
pH = –Log 0.830M
pH = 0.08
Therefore, the pH of the acid is 0.08