[H,o*] (M) [OH"] (M) pH Рон Sample Solution 101 10-15 -1 15 10° or 1 10-14 14 1 M HCI 10-1 acidic 10-13 13 10-2 gastric juice lime juice 10-12 12 10-3 1 M CH3CO,H (vinegar) stomach acid 10-11 11 10-4 10-10 wine 4 10 10-5 10-9 orange juice coffee 10-6 10-8 6. 8 rain water 10-7 10-7 pure water 10-8 10-6 neutral 8. 6. blood 10-9 ocean water baking soda 10-5 9. 10-10 104 10 4 10-11 10-3 11 Milk of Magnesia 3 10-12 10-2 12 2 household ammonia, NH, 10-13 10-1 13 bleach 10-14 10° or 1 14 1 M NaOH 10-15 101 basic 15 -1 LO 3. LO 4. What would be an appropriate indicator to use to measure the endpoint volume for a titration with a pH of 4.32 at the equivalence point? HINT: See Figure 14.22 (page 821) in your chemistry lecture textbook.

[H,o*] (M) [OH"] (M) pH Рон Sample Solution 101 10-15 -1 15 10° or 1 10-14 14 1 M HCI 10-1 acidic 10-13 13 10-2 gastric juice lime juice 10-12 12 10-3 1 M CH3CO,H (vinegar) stomach acid 10-11 11 10-4 10-10 wine 4 10 10-5 10-9 orange juice coffee 10-6 10-8 6. 8 rain water 10-7 10-7 pure water 10-8 10-6 neutral 8. 6. blood 10-9 ocean water baking soda 10-5 9. 10-10 104 10 4 10-11 10-3 11 Milk of Magnesia 3 10-12 10-2 12 2 household ammonia, NH, 10-13 10-1 13 bleach 10-14 10° or 1 14 1 M NaOH 10-15 101 basic 15 -1 LO 3. LO 4. What would be an appropriate indicator to use to measure the endpoint volume for a titration with a pH of 4.32 at the equivalence point? HINT: See Figure 14.22 (page 821) in your chemistry lecture textbook.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Determine the pH during the titration of 14.4 mL of 0.130 M perchloric acid by 7.26E-2 M sodium hydroxide at the following points:a. Before the addition of any sodium hydroxide b. After the addition of 12.9 mL of sodium hydroxide c. At the equivalence point d. After adding 33.5 mL of sodium hydroxide
Can you help me with this?
the pH at the equivalence point MISSED THIS? Read Section 18.4 (Pages 803 - 817) ; Watch_KCV 18.4A, IWE 18.6 . Express your answer as a whole number. Consider the titration of a 38.0 mL sample of 0.170 M HBr with 0.200 M KOH. Determine each of the following: pH = Submit Request Answer Part E the pH after adding 5.0 mL of base beyond the equivalence point Express your answer using two decimal places ? pH = Submit Request Answer
The next 9 questions are related to the titration of 20.00 mL of a 0.0750 M acetic acid solution with 0.0700 M KOH. How many mmol of the salt are present at the equivalence point? (ANALYTICAL AMOUNT, NOT EQUILIBRIUM AMOUNT)
Sketch an accurate titration curve by plotting pH as a function of mL of HCl added when a 40 mL solution of 0.100 M ammonia is titrated with 0.100 M HCl include pH values when:0mL of HCl is added, 10 mL, 20 mL, 30mL and 40 mL
a) Calculate the pH at each of the following points in the titration of 25.0 mL of 0.100 M NH3 with 0.0500 M HCl. Volume of HCl added: 0.0 mL, 25.0 mL, 50.0 mL, and 52.0 mL . b) Sketch the titration curve
Compare conductivity titration to the pH-metric titration that you performed earlier. Do both methods yield the same equivalence point? Explain.
Draw a titration curve for a strong acid titrated with a strong base. On the same axes draw a titration curve for a weak acid titrated with a strong base. Label the axes and explain differences in the curves.
In an acid-base neutralisation titration, equivalent quantities of hydronium and hydroxide ions are present Select one: a. At the beginning of the titration b. When the indicator changes colour c. Half way through the titration d. At the equivalence point
3. Calculate the pH at each of the following points in the titration of 50.00 ml of a 0.150M acetic acid using 0.275M NaOH. (Show work below.) (Ką = 1.8 x 105) (You can also refer to pages 792-794 from your textbook for help.) а. Initial pH: 0 ml of base added b. Halfway to equivalence point 5.00 mL before equivalence point С. d. At equivalence point e. 5.00 ml beyond equivalence point
What is the difference between equivalence point and end point on a titration curve. Illustrate.
If you allow your titration to go beyond a faint pink endpoint and it ends up dark pink what effect will that have on your calculated molarity of NaOH? Would you calculate a molarity that is too high to low or no different from the correct molarity