Strong Bases/Acids vs. Weak Bases/Acids The 4 Titration Curves Combinations NaOH + HCI Strong Base Strong Acid Strong Base+ Weak Acid HOOD HO+ HOEN Weak Base Strong Acid IOH + HO'HN NH.OH + CH.COOH Weak Base Weak Acid 4. Explain why the titrations which began with CH3COOH started from a higher pH value compared to those which began with HCI. 5. What was the purpose of adding the indicator to each titration? 6. Two titrations ended with the pH well above 10 the other two titrations ended with the pH below 10. Explain why this occurred.

Strong Bases/Acids vs. Weak Bases/Acids The 4 Titration Curves Combinations NaOH + HCI Strong Base Strong Acid Strong Base+ Weak Acid HOOD HO+ HOEN Weak Base Strong Acid IOH + HO'HN NH.OH + CH.COOH Weak Base Weak Acid 4. Explain why the titrations which began with CH3COOH started from a higher pH value compared to those which began with HCI. 5. What was the purpose of adding the indicator to each titration? 6. Two titrations ended with the pH well above 10 the other two titrations ended with the pH below 10. Explain why this occurred.

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

Bewis a titra on curve of a weak acid with NaOH. What region of the titration curve can the volume of NaOH at equivalence point be located? O с B A 2 A B Vol. NaOH (mL) 6 C 8 10
8. Suppose we titrate 24.0 mL of 0.100M HCIO4, a strong acid, with 0.100M NaOH, a strong base. Calculate the pH when a. 16.0 mL of NaOH is added b. 24.0 mL of NaOH is added 30.0 mL of NaOH is added c. HCIO4(aq) + NaOH(aq) NaCIO4(aq) + H2O(1)
A 150.0 mL sample of 0.20 M HF is titrated with 0.10 M NaOH. Determine the pH of the solution after the addition of 150.0 mL of NaOH. The Ka of HF is 3.5 × 10-4. Group of answer choices 4.33 3.46 3.15 4.15 2.08
Do 2
A chemistry student is asked to maked a buffer of pH = 4.0. Which of the following acids would be the best choice? Explain your selection to the best of your ability and in your own words. Formic acid -4 Ka = 1.8 x10 Acetic acid Ka = 1.8 x10-5 -5 Chloropropanoic acid Ka 7.8 x10 Benzoic acid Ka = 6.3 x10-5
Using the pH of the solution, a student determined that their hydroxide concentration was 0.1972 M. Which of the following standardized HCl dilutions would be most appropriate for their titration? 1.006×10−1M HCl 1.206×10−5M HCl 1.401×10−3M HCl 1.312×10−4M HCl 1.197×10−2M HCl
Ka(HOAC) = 1.8 x 10-5. A 1-L buffer solution is prepared by mixing 0.35 mol HOAC and 0.45 mol NaOAc. Which of the following processes will increase the pH of the above buffer solution? O a. add more water b.add more HOA c. add some HCI into the above buffer SO d. add some NH3 into the above buffer e. None of the above
A 650.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the pH of the solution before the addition of any KOH. The Ka of HF is 3.5 × 10-4. Group of answer choices 2.08 3.46 1.25 0.70 4.15
Consider the titration curve for a diprotic acid: 12 10 8 pH 6 4+ 2 + + 10 20 30 Volume of NaOH added (mL) Label the curve with the following items: first equivalence point, second equivalence point, first halfway point, halfway between first and second equivalence points. Determine K, and K, for this diprotic acid. al a2
The buffer was made by combining 0.220 M lactic acid (HC3H5O3) and 0.200 M sodium lactate ( NaC3H5O3). The Ka of HC3H5O3 is 1.4 x 10^-4. 1. write the equation describing the conjugate acid base relationship 2. Calculate the pH of the buffer 3. Calculate the pH of the buffer after the addition of 100.0 mL of 0.100 M potassium hydroxide to 0.9000 L of the buffer solution
You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (p?a=4.20) and 0.180 M sodium benzoate. How many milliliters of each solution should be mixed to prepare this buffer? benzoic acid: mL sodium benzoate: mL
Added strong base: NaOH solution OH Acetic acid/acetate buffer N-7 Mix OH +CH;COOH CH;COO" + H Added Weak acid in buffer cak base strong base Conjugate created from buffer CH.COOH What is the net ionic equation for the reaction that occurs when small amounts of sodium hydroxide are added to HOCI/NAOCI buffer solution? Na + HOCI O NAOH + HOCI NaCl + OH™ H2O + NaCl OH+ OCI HOCI + 02- OH +HOCI H2O + OCI" H + HOCI H2 + OC