Q 17 please d. 4.95 e. 2.8515. the pAg during the titration of 50.0 ml of 0.040 M NaCl with 20 ml of 0.100 AgNO3 (Ksp for AgCl = 1.82×10-10)a. 4.87b. 3.87c. 2.7616. 100 ml of city drinking water was buffered at pH 10. after addition of indicator the solution needed 15.46 ml of5.140×10 MEDTA for titration. the hardness of water in terms of ppm of CaCO, is .(MW of CaCO, is 100.08g/mlo)a. 110.4 ppmb. 79.5 ppmc. 114.33ppmd. 112.3 ppm e. 283.3 ppm17. A 50.0-mL sample containing Ni2+ was treated with 25.0 mL of 0.0500 M EDTA to complex all theNi2 and leave excess EDTA in solution. The excess EDTA was then back-titrated, requiring 5.00 mL of0.0500 M Zn². What was the concentration of Ni2+ in the original solution?d.5.23 ×104 Mb. 4.0×10 Ma. 2.0 × 10 Mc. 2.1 × 10-M18. The ApH for 20.0 mL of 0.1750 M formic acid solution (weak acid ka = 1.8x104) after it diluted with 45.0 mL ofdistilled water (the final volume of the acid is 65 ml ).a. 0.25b. 0.35c. 0.48d. 1.78e.2.3519. The molarity of a 22.75% HCI solution. The density of this solution is 1.13 g/mL, and the molar mass of HCI is36.46 g/mol.a. 26.7 Mc. 3.75 Mb.31.0 Me. none of thesed. 7.05 Me. 12.1 M20. 25.0 mL of NaCl unknown concentration was titrated against 23.0 mL of 0.009 M AgNO3. Calculate the ppm ofNaCl in the original sample. (Na-23 g/mol, Cl- 35.5 g/mol)d. 29.39ppm. e 950ppma. 484.38ppmb. 293.94ppmc. 48.44ppm21. 100 ml of city drinking water was buffered at pH 10. after addition of indicator the solution needed 21.46 ml of5.140×10-3 M EDTA for titration. the hardness of water in terms of ppm of CaCO3 is. (MW of CaCO3 is 100.08g/mlo)a) 110.4 ppmb) 1104.04 ppmc) 114.33ppmd. 234.45 pp e) never of theses22. The pH of of 0.1 00M NaHCO, solution is (the dissociation constants for H₂CO3 is kal = 4.45 × 107 and Ka2=4.69 × 10-¹¹)a)8.33b) 8.63c) 9.8d) 10.6723. A silver nitrate solution contains 14.77 g of primary-standard AgNO3 (169.87 g/mol) in 1.00 L. What volumeof this solution will be needed to react completely with 0.2631 g of NaCl (58.44 g/mol)?a)51.78 ml.b) 0.05231 Lc) 0.543 mld) 53.657 mle. 26.36 mle.5.3

We have find out the concentration of Ni2+ in the original solution.

a. 110.4 ppm b. 79.5 ppm 17. A 50.0-mL sample containing Ni2+ was treated with 25.0 mL of 0.0500 M EDTA to complex all the Ni²+ and leave excess EDTA in solution. The excess EDTA was then back-titrated, requiring 5.00 mL of 0.0500 M Zn². What was the concentration of Ni2+ in the original solution? a. 2.0 × 10 M b. 4.0 × 10 M c. 2.1 ×10-M d.5.23 x 104 M e. none of these

a. 110.4 ppm b. 79.5 ppm 17. A 50.0-mL sample containing Ni2+ was treated with 25.0 mL of 0.0500 M EDTA to complex all the Ni²+ and leave excess EDTA in solution. The excess EDTA was then back-titrated, requiring 5.00 mL of 0.0500 M Zn². What was the concentration of Ni2+ in the original solution? a. 2.0 × 10 M b. 4.0 × 10 M c. 2.1 ×10-M d.5.23 x 104 M e. none of these

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 74QAP: Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a)...

See similar textbooks

Similar questions

When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
A buffer is prepared using the butyric acid/butyrate (HC4H7O2/C4H7O2)acid-base pair. The ratio of acid to base is 2.2 and Ka for butyric acid is1.54105. (a) What is the pH of this buffer? (b) Enough strong base is added to convert 15% of butyric acid to the butyrate ion. What is the pH of the resulting solution? (c) Strong acid is added to the buffer to increase its pH. What must the acid/base ratio be so that the pH increases by exactly one unit (e.g., from 2 to 3) from the answer in (a)?
K4 for acetic acid is 1.7 105 at 25C. A buffer solution is made by mixing 52.1 mL of 0.122 M acetic acid with 46.1 mL of 0.182 M sodium acetate. Calculate the pH of this solution at 25C after the addition of 5.82 mL of 0.125 M NaOH.
A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric acid. Assume no volume change after NaF is added. Calculate the pH of this buffer.
A buffer solution is composed of 1.360 g of KH2PO4 and 5.677 g of Na2HPO4. (a) What is the pH of the buffer solution? (b) What mass of KH2PO4 must be added to decrease the buffer solution pH by 0.50 unit from the value calculated in part (a)?
Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
The weak base propylamine (CH3(CH2)2NH2) has a Kb = 4.7 x10-4. It can be used in some pharmaceuticals and pesticides. A 25.0 mL sample of 0.185 M propylamine solution was titrated with 0.120 M HCl. What is the pH of this solution at the equivalence point? A. 2.23 B. 5.90 C. 2.03 D. 5.70 E. 5.74
In the titration of 50.00 mL 0.0200M weak base B using 0.0150 M HCI, which indicator is the best one to be used? (pK, of the weak base B is 10.50). Indicator 4: Thymolthalein: pH transition = 8.5-10.5 OIndicator 5: Indigo Carmine: pH transition= 11.6- 14.0 Indicator 3: Cresol red: pH transition 7.2-8.8 Indicator 1: Cresol purple: pH transition = 1.2-2.8 Indicator 2: Methyl red: pH transition = 4.8-6.0
A 24.0 mL sample of 0.115 M sulfurous acid (H,S03) is titrated with 0.1019 M KOH At what added volume of base solution does the first equivalence point occur? Express your answer in mililiters to three significant figures. V. mL Submit Request Answer Vorue nertlel
In the titration of Y(OH)3 with HX, which of the following equations should be used to calculate the concentration of Y(OH)3? 3M.•V. HX 'Y(0H), M. Y(OH); V HX а. M....•V *HX'HX M. Y(OH); V. Y(OH), 3 b. M..V. Hx'Y(OH), 1 M. Y(OH)3 V. HX 3 с. 3M..•V. HX 'HX Y(OH); d. My(OH), V. Y(OH), ||
O *17.61 Calculate the solubility of Mn (OH)₂ in grams per liter when buffered at pl a. 7.0, b. 9.5, c. 11.8.
Question 1 Derive the Henderson-Hasselbalch equation for the dissociation of a weak base, B, in terms of pOH and pKb. 12pt Paragraph V р Question 2 BI T² v V (mL) 0.00 ...: i 0 words A 0.5892 g of an Acetylsalicylic Acid (a monoprotic acid, FW 192.14) sample was titrated with a 0.1273 M standard NaOH solution. The titration data is given. C₂ pH 2.79