A 75.0-ml. sample of 0.0650 MHCN (K -62 x 10-19) is titrated with 065 M NaOH....
Question 2 (10 points) If 25.0 mL of 0.451 M NaOH solution is titrated with 0.253 MH2SO4, the flask at the endpoint will contain (besides the indicator phenolphthalein) as the principal components: sodium hydroxide, sulfuric acid, and water dissolved sodium sulfate and water sodium hydroxide, sodium sulfate, and water dissolved sodium sulfate, sulfuric acid, and water precipitated sodium sulfate and water Question 3 (10 points) A 75.0-ml sample of 0.0650 MHCN (K-62 10-10) is titrated with 0.65 M NaOH. What...
A 75,0 mL sample of 0.0500 MHCN (K-6.2 x10-10) is titrated with 0.421 M NaOH to the equivalent point. What is pH of the solution at equivalent point? (Hint: don't forget to find the total volume of the solution.) A 2.57 B. 14 10.9 D.7 E none of these
Part C A 75.0-mL volume of 0.200 M NH3 (Kb = 1.8 x 10-5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 15.0 mL of HNO3 . Express your answer numerically. Part D A 52.0-mL volume of 0.35 M CH3COOH (Ka = 1.8 x 10-5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 19.0 mL of NaOH. Express your answer numerically.
8. [-/19 Points] DETAILS 27.0 mL of 0.160 M HClO is titrated with 0.140 M NaOH. a) What volume of base is required to reach the equivalence point? volume of base = mu b) What is the pH of the solution after addition of 15.5 mL of base? pH = c) What is the pH of the solution after addition of 33.4 mL of base? pH = d) What is the pH at the equivalence point? рн
A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10-5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 11.0mL of HNO3.A 52.0-mL volume of 0.35 M CH3COOH (Ka=1.8×10-5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 31.0mL of NaOH.
2. 20.00 mL of 0.270 M HA (K. = 7.2 x 10-4) was titrated with 0.300 M sodium hydroxide (3 + 3 + 2 + 3 + 3 + 3 + 12 = 29 points) a) Write the titration equation and calculate volume of NaOH needed to reach the equivalence point. ml b) At what volume of the titrant would pH=pKa? Why? c) pH at the equivalence point when the acid and base are neutralized will be ..choose one of...
A student titrated a 100.0 mL sample of 0.100 M acetic acid with 0.050 M NaOH. (For acetic acid, Ka = 1.8 * 10^-5 at this temperature.) (a) Calculate the initial pH. (b) Calculate the pH after 50.0 mL of NaOH has been added. (c) Determine the volume of added base required to reach the equivalence point. (d) Determine the pH at the equivalence point?
Titrations Part A A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10−5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 19.0 mL of HNO3. Express your answer numerically. Part B A 52.0-mL volume of 0.35 M CH3COOH (Ka=1.8×10−5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 23.0 mL of NaOH. Express your answer numerically.
a 25.00 ml sample of a weak acid is titrated with 0.225 M NaOH. a total of 12.20 ml of the NaOH is required to reach the equivalence point where the pH is 9.96. determine the value of pka for this weak acid
45.00 mL of a 0.250 M H2SO4 solution is titrated with 0.100 M NaOH. a. What is the chemical equation that describes this neutralization reaction? b. What is the volume in mL of NaOH required to reach the equivalence point? c. At the equivalence point, what are the sodium and sulfate ion concentrations? d. At the equivalence point, what are the pH and pOH