Incorrect Question 3 0/ 0.5 pts Which statement best explains why the pH at the equivalence point of the titration of a strong acid with a strong base is 7.0 (at or near 25 °C)? A basic salt is formed, but it is neutralized by excess strong acid. All analyte has been consumed. An acidic salt is formed, but it is neutralized by excess strong base. There is no excess titrant. A neutral salt is the only chemical species present.

Incorrect Question 3 0/ 0.5 pts Which statement best explains why the pH at the equivalence point of the titration of a strong acid with a strong base is 7.0 (at or near 25 °C)? A basic salt is formed, but it is neutralized by excess strong acid. All analyte has been consumed. An acidic salt is formed, but it is neutralized by excess strong base. There is no excess titrant. A neutral salt is the only chemical species present.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.84QE: Phenolphthalein is a commonly used indicator that is colorless in the acidic form (pH 8.3) and pink...

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1. Calculate [H+], [OH-], pH and pOH of:a. 0.1 M HNO3 b. 2.00 M (weak acid) HF (Ka=6.8 x 10^-4) 2. In the preparation of the standard curve for protein analysis, 50 mnBSA (bovine serum albumin) dissolved in H2O to a final volume of 5mL was used as stock solution. What is the weight of BSA in 0.1 mL ofstock solution? In 0.2 mL? 3. . The above mentioned aliquots (#9) which were diluted with enoughwater to a final volume of 1 mL were assayed colorimetrically andyielded the following absorbance readings:mL stock mL H2O Absorbance0.2 0.8 0.1000.4 0.6 0.2000.6 0.4 0.3000.8 0.2 0.4001.0 0.0 0.500 i. Tabulate mg BSA vs. absorbance readingii. Draw the curve where mg BSA is on x-axis and absorbance ony-axis (use graphing paper).iii. Calculate the slope of the curveiv. If a sample solution has an…
Limestone consists mainly of the mineral calcite, The carbonate content of 0.541 3 g of powdered limestone was measured by suspending the powder in water, adding 10.00 mL of 1.396 M HCl, and heating to dissolve the solid and expel Calcium carbonate FM 100.087 The excess acid required 39.96 mL of 0.100 4 M NaOH for complete titration to a phenolphthalein end point. Find the weight percent of calcite in the limestone
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Titration of unknown acid with NaOH. Determine the pKa of unknown acid: mass H2A=0.5 g H2O=50 mL Volume @ eq point: 23.7 mL NaOH= 0.2084M pH @ Veq = 7.9 H2A+H2O <---->[HA-]+[H3O+]
A 0.3012g sample of an unknown monoprotic acid requires 24.13mL of 0.0944MNaOH for neutralization to a phenolphthalein end point. There are 0.32mL of 0.0997MHCl used for back titration. a. How many moles of OH are used? How many moles of H+ from HCl? _______moles OH ________moles H+ b. How many moles of H+ are there in the solid acid? Use Eq.5. ____________ moles H+ in solid c. What is the molar mass of the unknown acid? Use Eq.4. ____________ g/mol
Phenolphthalein is a commonly used indicator that is colorless in the acidic form (pH 8.3) and pink in the base form (pH 10.0). It is a weak acid with a pKa of 8.7. What fraction is in the acid form when the acid color is apparent? What fraction is in the base form when the base color is apparent?
Titration of 15.00 mL of a weak, monoprotic acid solution requires 22.84 mL of a 0.09837M standardized NaOH solution. What is the molarity of the acid solution?(Show your work.)
If a water has a carbonate alkalinity of 120.00 mg/L as the ion and a pH of 10.30, what is the bicarbonate alkalinity in mg/L as the ion? The answer is HCO_3=130.686 or 130.7 mg/LPlease do explain the steps
Which of the following accurately describes the pKA of acetic acid (CH3COOH)? Select all that are applicable. a.pKA = pH at the steepest point on the titration curve b.pKA = pH at the equivalence point volume on the titration curve c.pKA = pH when [CH3COOH] = [CH3COO-] in solution d.pKA = pH at the shallowest point on the titration curve e.pKA = pH at the half-equivalence point volume on the titration curve f.pKA =pH when [H3O+] = [OH-] in solution
Tony is showing a bacterium having high pH requirement for its growth. He then has to prepare a minimal medium at pH 9. Adding 0.5 ml of the pH indicator to 10 ml of the medium, the solution remained colorless. The pH of the medium was adjusted using 2.25 ml of the 0.05 N titrant. a. What was the pH indicator utilized? b. What is the amount of 1 N titrant needed to adjust 150 ml of minimal medium to pH 9? c.What was the titrant he used?
The data from my observations is given below: Concentration of Standardized NaOH - 1.00 mol/L Mass concentration of acetic acid - 2.40 g/L Trial 1 Trial 2 Measured pH of the acetic acid solution 3.07 3.05 Mass of acetic acid solution taken for titration 20.0 g 20.0 g Initial buret reading of NaOH titrant 0.00 mL 0.00 mL Final buret reading of NaOH titrant 0.82 mL 0.79 mL Net volume of NaOH 0.82 mL 0.79 mL Millimoles of NaOH to end point of titration 0.82 mmol 0.79 mmol Millimoles of acetic acid in sample 0.82 mmol 0.79 mmol Molar concentration of acetic acid solution 0.043 mol/L 0.041 mol/L Calculated molar mass of acetic acid g/mol g/mol Average molar concentration of acetic acid for the samples titrated: 0.042 mol/L Average pH: 3.06 Question: Calculate the corresponding [H3O+], compute the corresponding concentration of A- and HA, and calculate the dissociation constant Ka Thank you!