🤓 Based on our data, we think this question is relevant for Professor Harwood's class at UNI.
1) At start of titration:
• When getting the pH of a strong acid solution (HNO3):
1) pH = 0.903
Reaction: HCl(aq) + NaOH(aq) → H2O(l) + NaCl(aq)
moles HNO3 = 0.0025 mol HNO3
moles NaOH = 0.00225 mol NaOH
moles NaOH < moles HNO3 → pH depends on molarity of acid (NaOH is consumed)
7.14 x 10-3 M
2) pH = 2.15
A 20.0-mL sample of 0.125 M HNO3 is titrated with 0.150 M NaOH. Calculate the pH for at least five different points throughout the titration curve and make a sketch of the curve.
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Based on our data, we think this problem is relevant for Professor Harwood's class at UNI.