Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Titration of (4.890x10^-1) grams of monoprotic weak acid (dissolved in KCl) required (2.44000x10^1) mL of (2.12000x10^-1) molar NaOH solution to reach equivalence. Based on this information, how many moles of weak acid are present in this solution?
Format your answer with correct number of sig figs. Use scientific notation.
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- Explain the difference between an indicator endpoint for a titration analysis and the true equivalence point for the titration. Please simplify the answer so I can understand. Thanksarrow_forwardTitus titrates 45 mL of 0.750 M lactic acid (HC₂H₂O², Ka NaOH. = 1.5 × 104) using 0.250 M Calculate the pH of the resulting solution at each of the following points in the titration. After adding 24.750000000000004 mL of the NaOH solution: At the equivalence point: After adding 191 mL of the NaOH solution:arrow_forwardIn an acid-base titration, a base or acid is gradually added to the other until they have completely neutralized each other. Since acids and bases are usually colorless (as are the water and salt produced in the neutralization reaction), pH is measured to monitor the reaction. Suppose that the equivalence point is reached after approximately 393 mL of a NaOH solution has been added (enough to react with all the acetic acid present) but that replicates are equally likely to indicate from 373 to 417 mL (exclusive), measured to the nearest mL. Assume that two technicians each conduct titrations independently. What is the probability that the average volume at equivalence from the technicians is 416 mL or 417? Select one: O a. 0.79069767 b. 0.00000000 c. 0.00054083 d. 1.00000000 e. 0.00049383 f. 0.02941176 O g. 0.04651163 O Oarrow_forward
- 1) Determine the pH during the titration of 74.5 mL of 0.348 M nitrous acid (Ka = 4.5×10-4) by 0.348 M NaOH at the following points. (a) Before the addition of any NaOH ? (b) After the addition of 18.0 mL of NaOH ? (c) At the half-equivalence point (the titration midpoint) ? (d) At the equivalence point ? (e) After the addition of 112 mL of NaOH ?arrow_forwardThe half‑equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.500 moles of a monoprotic weak acid (?a=8.9×10−5) is titrated with NaOH, what is the pH of the solution at the half‑equivalence point? pH= ( Please type answer note write by hend )arrow_forwardWhat is the pH at the equivalence point in the titration of 60.00 mL of 0.200 M HA (a generic acid with K, = (2.26x10^-5)) with 0.400 M NaOH? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 Answerarrow_forward
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- A 150 mL solution of NaOH is titrated with HI. Phenol red is the indicator, which is red at high pH values and yellow at low pH values. The indicator be [ Select ] when you first put it into your analyte, before any titrant is added. The indicator will be [ Select] at the endpoint. The indicator will be [Select] V if you overshoot the endpoint and add too much acid.arrow_forwardConstruct a graph and plot the titration curve for a 10.0 mL aliquot of 0.100 mol/L NH3 (pKb=4.74) with 0.100 mol/L HCl. For this purpose, make a table with nine added volumes of HCl solution, which you consider adequate, with the corresponding pH value. Write the development of all calculations and use approximate formulas.arrow_forward
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