HF is a weak acid, NaOH is a strong base. At the equivalence point, HF and NaOH are fully reacted to give NaF, which is the salt of weak acid and strong base.
HF (aq) + NaOH (aq) = NaF (aq) + H2O (l)
A salt of weak acid and strong base has basic pH ( that is, pH more than 7). For, the answer is false.
( similarly, salt of strong acid weak base has pH less than 7, and salt of strong acid strong base has pH = 7)
When HF(aq) is titrated with NaOH(aq), the pH at the equivalence point is less than 7.0....
HF is a weak acid (a monoprotic one). When HF is titrated with a strong base (like NaOH), it will eventually reach an equivalence point where exactly all of the HF has been reacted with exactly the needed amount of NaOH. What will the pH be when HF reaches equivalence point? (Hint: think about what products will be present and whether they are weak acids, weak bases or neutral...) pH will be 7.0 pH will be greater than 7.0 pH...
What is the pH at equivalence point when HCl(aq) is titrated with NaOH(aq) at 25 °C? 7 1 14 0
What is the pH of the analyte in a titration at the equivalence point when a 10.00 mL aliquot of 0.25 M HF ( Ka = 3.5 x 10-4, pKa = 3.46) is titrated with 0.10 M NaOH? 8.23 8.15 7.00 5.85
An acid-base titration is performed: 250.0 mL of an unknown concentration of HCl(aq) is titrated to the equivalence point with 36.7 mL of a 0.1000 M aqueous solution of NaOH. Which of the following statements is not true of this titration? A. At the equivalence point, the OH−concentration in the solution is 3.67×10−3 M. B. The pH is less than 7 after adding 25 mL of NaOH solution. C. The pH at the equivalence point is 7.00. D. The HCl...
What is the pH of when 0.047 L of 0.0082 M HCN is titrated to its equivalence point with 0.085 L of NaOH? The Ka of HCN is 4.9×10–10.
1. When titrating of an acid of HF and Ca(OH) 2 , the PH at equivalent point: A. pH will be less than 7 at the equivalence point. B. pH will be greater than 7 at the equivalence point. C. titration will require more moles of base than acid to reach the equivalence point. D. pH will be equal to 7 at the equivalence point. E. titration will require more moles of acid than base to reach the equivalence point....
What is the pH of when 0.019 L of 0.0040 M HCN is titrated to its equivalence point with 0.098 L of NaOH? The Ka of HCN is 4.9x10-10 Multiple tries are permitted; however, 20% (1 /5 ) point will be deducted for each incorrect response
A 35.00-mL solution of 0.2500 M HF is titrated with a standardized 0.2029 M solution of NaOH at 25° C. (a) What is the pH of the HF solution before titrant is added? (b) How many milliliters of titrant are required to reach the equivalence point? mL (c) What is the pH at 0.50 mL before the equivalence point? (d) What is the pH at the equivalence point? (e) What is the pH at 0.50 mL after the equivalence point?
A 35.00−mL solution of 0.2500 M HF is titrated with a standardized 0.1825 M solution of NaOH at 25°C. Be sure to answer all parts. A 35.00-mL solution of 0.2500 M HF is titrated with a standardized 0.1825 M solution of NaOH at 25° C. (a) What is the pH of the HF solution before titrant is added? 1.9 (b) How many milliliters of titrant are required to reach the equivalence point? mL (e) What is the pH at 0.50...
1) NaOH(aq) + HCl(aq) - NaCl(aq) + H2O(1) To determine the concentration of a NaOH(aq) solution, a student titrated a 50. mL sample with 0.10 M HCl(aq). The reaction is represented by the equation above. The titration is monitored using a pH meter, and the experimental results are plotted in the graph below. 13. 0S 7.04 Answer Key on School Loop @ P 1.07. 0 25.0 50.0 Volume HCI added (mL) One student titrated the NaOH(aq) with 1.0 M HCl(aq)...