Answered: What is the pH of a 0.015 M aqueous…

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What is the pH of a 0.015 M aqueous solution of barium hydroxide? Select one: a. 1.52 b. 12.25 c. 1.82 d. 12.48

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.17QAP

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A quantity of 0.15 M hydrochloric acid is added to a solution containing 0.10 mol of sodium acetate. Some of the sodium acetate is converted to acetic acid, resulting in a final volume of 650 mL of solution. The pH of the final solution is 4.56. a What is the molar concentration of the acetic acid? b How many milliliters of hydrochloric acid were added to the original solution? c What was the original concentration of the sodium acetate?
What is a salt? List some anions that behave as weak bases in water. List some anions that have no basic properties in water. List some cations that behave as weak acids in water. List some cations that have no acidic properties in water. Using these lists, give some formulas for salts that have only weak base properties in water. What strategy would you use to solve for the pH of these basic salt solutions? Identify some salts that have only weak acid properties in water. What strategy would you use to solve for the pH of these acidic salt solutions? Identify some salts that have no acidic or basic properties in water (produce neutral solutions). When a salt contains both a weak acid ion and a weak base ion, how do you predict whether the solution pH is acidic, basic, or neutral?
Two samples of 1.00 M HCl of equivalent volumes are prepared. One sample is titrated to the equivalence point with a 1.00 M solution of sodium hydroxide, while the other sample is titrated to the equivalence point with a 1.00 M solution of calcium hydroxide. a Compare the volumes of sodium hydroxide and calcium hydroxide required to reach the equivalence point for each titration. b Determine the pH of each solution halfway to the equivalence point. c Determine the pH of each solution at the equivalence point.
A solution is prepared from 0.150 mol of formic acid and enough water to make 0.425 L of solution. a Determine the concentrations of H3O+ and HCOO in this solution. b Determine the H3O+ concentration that would be necessary to decrease the HCOO concentration above by a factor of 10. How many milliliters of 2.00 M HCl would be required to produce this solution? Consider that the solution was made by combining the HCl, the HCOOH, and enough water to make 0.425 L of solution. c Qualitatively, how can you account for the differences in the percentage dissociation of formic acid in parts a and b of this problem?
Strong Acids, Weak Acids, and pH Two 0.10-mol samples of the hypothetical monoprotic acids HA(aq) and HB(aq) are used to prepare 1.0-L stock solutions of each acid. a Write the chemical reactions for these acids in water. What are the concentrations of the two acid solutions? b One of these acids is a strong acid, and one is weak. What could you measure that would tell you which acid was strong and which was weak? c Say that the HA(aq) solution has a pH of 3.7. Is this the stronger of the two acids? How did you arrive at your answer? d What is the concentration of A(aq) in the HA solution described in part c? e If HB(aq) is a strong acid, what is the hydronium-ion concentration? f In the solution of HB(aq), which of the following would you expect to be in the greatest concentration: H3O+(aq), B(aq), HB(aq), or OH(aq)? How did you decide? g In the solution of HA(aq), which of the following would you expect to be in the greatest concentration: H3O+(aq), A+(aq), HA(aq), or OH(aq)? How did you decide? h Say you add 1.0 L of pure water to a solution of HB. Would this water addition make the solution more acidic, make it less acidic, or not change the acidity of the original solution? Be sure to fully justify your answer. i You prepare a 1.0-L solution of HA. You then take a 200-mL sample of this solution and place it into a separate container. Would this 200 mL sample be more acidic, be less acidic, or have the same acidity as the original 1.0-L solution of HA(aq)? Be sure to support your answer.
The pH of Mixtures of Acid, Base, and Salt Solutions a When 0.10 mol of the ionic solid NaX, where X is an unknown anion, is dissolved in enough water to make 1.0 L of solution, the pH of the solution is 9.12. When 0.10 mol of the ionic solid ACl, where A is an unknown cation, is dissolved in enough water to make 1.0 L of solution, the pH of the solution is 7.00. What would be the pH of 1.0 L of solution that contained 0.10 mol of AX? Be sure to document how you arrived at your answer. b In the AX solution prepared above, is there any OH present? If so, compare the [OH] in the solution to the [H3O+]. c From the information presented in part a, calculate Kb for the X(aq) anion and Ka for the conjugate acid of X(aq). d To 1.0 L of solution that contains 0.10 mol of AX, you add 0.025 mol of HCl. How will the pH of this solution compare to that of the solution that contained only NaX? Use chemical reactions as part of your explanation; you do not need to solve for a numerical answer. e Another 1.0 L sample of solution is prepared by mixing 0.10 mol of AX and 0.10 mol of HCl. The pH of the resulting solution is found to be 3.12. Explain why the pH of this solution is 3.12. f Finally, consider a different 1.0-L sample of solution that contains 0.10 mol of AX and 0.1 mol of NaOH. The pH of this solution is found to be 13.00. Explain why the pH of this solution is 13.00. g Some students mistakenly think that a solution that contains 0.10 mol of AX and 0.10 mol of HCl should have a pH of 1.00. Can you come up with a reason why students have this misconception? Write an approach that you would use to help these students understand what they are doing wrong.
When 10 mL of 0.1 M NaOH is added to 50 mL of 0.05 M HCl solution, which of the following is the final pH of the solution?A. 7.00B. 9.90C. 10.12D. 1.60
6. A stock solution of barium hydroxide was prepared by dissolving 4.71 g of barium hydroxide in 550. mL of water. A 63.0 mL portion of the stock solution was taken and diluted by adding 47.0 mL of water. Calculate the pH of the dilute solution
Will 260.0 milligrams of calcium carbonate raise the pH of 75.0 milliliters of stomach fluid from a low pH of 1.00 into the normal pH range of 1.50-3.50? In the last discussion, you calculated that 260.0mg of calcium carbonate is 0.2600g of calcium carbonate. The next step is to figure out the formula of calcium carbonate and to calculate the molar mass of calcium carbonate in grams per mole. Submit a reply that that tells how you decided to approach the problem and shows the work that results in an answer. Use correct units and significant figures and correct symbols for elements and math. In addition, select another student's explanation that makes sense to you and reply with a comment about the insight you gained from their answer. Calcium carbonate is an ionic compound. Ionic nomenclature is in section 2.8. Molar mass is described on page 74 in section 2.8 of the textbook.
2.) A 3.90 g sample of aniline (C.HSNH2, Kp = 4.3 x 10" at 25°C) is dissolved in sufficient water to prepare 100. mL solution. Which is the pH of this solution? A. 4.87 В. 9.13 С. 9.74 d. 10.74 Keywords: amine, weak base, pH, pOH, base-ionization constant (KB), molarity, molar mass, RICE table, conjugate acid, conjugate base, Kú expression. Concepts: Calculation of weak base pH 10:12 PM
29. What volume of a 5.0 M CaCl2 solution do you need to make 1.0 L of a 0.1 M CaCl2 solution? 30. Use the ideal gas law to determine what is the volume of 10.0 moles of gas under 5.0 atm of pressure at a temperature of 200.0 degrees Celsius? Keep track of significant figures! 31. 1 mole of ANY ideal gas has the same volume at room temperature and atmospheric pressure. T / F 32. If an ideal gas is held at constant temperature and the pressure is increased, the volume of the gas: a. increases b. does not change c. decreases 33. What are the spectator ions from the following reaction? AgNO3(aq) + MgCl2(aq) → ? a. Mg2+ and CI b. Ag* and Cl c. Mg²+ and NO3 d. Ag* and Cl 34. AG = AH -TAS is the equation for the Gibbs free energy of reaction for a chemical process. If the AG for a reaction is negative, the reaction can proceed to the products. T/F 35. AG = AH -TAS is the equation for the Gibbs free energy of reaction for a chemical process. If the AH for a reaction is positive and the AS is…
A solution containing 2.60 x 10-3 moles of NAOH and 3.32 x 10-3 moles of HCl into a container and then water is added until the final volume is 1.00 L. What is the pH of this solution? (Hint: pH + pOH=14; pH= -log1o [H"] and pOH = -log10 [OH"]) OA. 2.84 О в. 10.86 Oc 11.16 O D. 3.14 O E. 2.50

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