Below are descriptions of two pH titration curves, labeled c and d:**Graph c:**- The graph illustrates a titration curve where the pH decreases as the volume increases.- Initial pH starts high around 13 and decreases gradually until a sharp drop occurs.- The sharp decline begins around a volume of 20 units and levels off near a pH of 2.- This graph typically represents the titration of a strong base with a strong acid, where the equivalence point causes a rapid decline in pH.**Graph d:**- This graph shows a titration curve where the pH increases with increasing volume.- Starting at a low pH around 1, it rises steadily before a sharp increase occurs.- The sharp rise begins near a volume of 20 units, leveling off around a pH of 11-12.- This is characteristic of a strong acid titrated with a strong base, where the pH rises dramatically as the solution reaches neutrality and beyond.Both graphs display the relationship between pH and volume, showcasing the dramatic change at the equivalence point typical of strong acid-strong base titrations. ### Acid-Base Titration Exercise**Objective**: Match the following acid-base titration plots with the correct titrant and sample.**Given**: Equivalence volume, $ V_{\text{eq}} = 20.00 \, \text{mL} $**Options**:1. Titrant: Strong Acid; Sample: Strong Base2. Titrant: Strong Base; Sample: Strong Acid3. Titrant: Strong Acid; Sample: Weak Base4. Titrant: Strong Base; Sample: Weak Acid**Graphs**:#### Plot a:- **Graph Description**: - The graph shows pH on the y-axis and volume on the x-axis. - Initial high pH around 12-13. - Gradual decrease until a sharp drop near $ V_{\text{eq}} = 20.00 \, \text{mL} $. - Final pH drops towards 1-2.- **Interpretation**: - This indicates the titration of a strong base by a strong acid.#### Plot b:- **Graph Description**: - The graph shows pH on the y-axis and volume on the x-axis. - Initial low pH around 2-3. - Gradual increase until a sharp rise near $ V_{\text{eq}} = 20.00 \, \text{mL} $. - Final pH rises towards 12-13.- **Interpretation**: - This indicates the titration of a strong acid by a strong base.**Matching**:1. Plot a matches with Option 1: Titrant: Strong Acid; Sample: Strong Base2. Plot b matches with Option 2: Titrant: Strong Base; Sample: Strong Acid

The question is based on the concept of titrations. We need to identify the nature of acid and base…

2 Match the following acid-base titration plots with the correct titrant and sample. Veg = 20.00 mL (1) Titrant: Strong Acid; Sample: Strong Base (2) Titrant: Strong Base; Sample: Strong Acid (3) Titrant: Strong Acid; Sample: Weak Base (4) Titrant: Strong Base; Sample: Weak Acid a. b. 13 ITU 10 15 Volume 12 11 10 9 8 9 6 5 4 3 2 1 0 14 13 12 11 10 9 8 7 6 5 4 3 2 1 0 0 0 5 5 10 15 Volume 20 20 25 25 30 30

2 Match the following acid-base titration plots with the correct titrant and sample. Veg = 20.00 mL (1) Titrant: Strong Acid; Sample: Strong Base (2) Titrant: Strong Base; Sample: Strong Acid (3) Titrant: Strong Acid; Sample: Weak Base (4) Titrant: Strong Base; Sample: Weak Acid a. b. 13 ITU 10 15 Volume 12 11 10 9 8 9 6 5 4 3 2 1 0 14 13 12 11 10 9 8 7 6 5 4 3 2 1 0 0 0 5 5 10 15 Volume 20 20 25 25 30 30

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...

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hi, can you reexplain the 0.6149 g * 1 mol KHP204.22 g= 0.003011 mol KHP Moles of KHP(KHC8H4O4) used in second titration = 0.003011 mol (Answer)
A The graph shows the titration curves of a strong acid and a weak acid. Estimate the pk, of the weak acid from its titration curve V 14 12 10 pH 12086420 Volume of strong base (ml) 1st attempt Write the estimated pK, to one decimal place 1 OF 8 QUESTIONS COMPLETED 82 W S # 3 Z X E 80 FI D $ 4 C R F K5 V 4 FS T G A 6 B S Y 27 & H 8 U N 8 00 DHI 14 M 9 K TV O hi See Periodic Table O L SUBMIT ANSWER P ** FIL
culate the pH during the titration gent. The Ka of acetic acid is 1.75x105. 801031 1801031/ A) 10.00 C) 191801031 of 50.00 191801031 191801031 19 E) 8.73 191801031 1 m of 0.100 M acetic acid with 0.1000 M sodium hydroxide at 25°C after the addition of 25.00 mL of 191801031 91801031 191801031 191801031 191801031 191801031 191801031 031 191801001 031 191801031 191801031 101801031 031 191801031 191801031 191801031 191801031 191801031 101801031 (91801031 101801031 191801031 191801031 191801031 191801031 191801031 191801031 191801031 19180103 191801031 101001031 191801031 191801031 181801031 191801031 181801004 391 191301051 19
10:49 1 4 7 +/- Question 6 of 10 In the titration of 69.0 mL of 0.400 M HCOOH with 0.150 M LIOH, how many mL of LiOH are required to reach the equivalence point? 2 5 8 mL 3 60 9 O Submit Tap here or pull up for additional resources XU x 100