Lareina the laboratory technician is given the task of making a solution containing HOBr ( Ka = 2.8 x 10 ⁹) and KOBr and testing its behavior when strong acid or base is added to it. Part 1 First, Lareina combines 82.86 g KOBr and 250 mL of 1.50 M HOBr, and adds enough distilled water to make 925 mL of solution. What is the pH of this solution? pH solution= Part 2 Next, Lareina adds 16.0 mL of 2.20 M HNO3 to 350 mL of the solution made in Part 1. What is the pH of the solution after the HNO, is added? pH after HNO, added = Part 3 Finally, Lareina 16.0 mL of 2.00 M NaOH ito 395 mL of the solution made in Part 1. What is the pH of the solution after the NaOH is added? pH after NaOH added =

Lareina the laboratory technician is given the task of making a solution containing HOBr ( Ka = 2.8 x 10 ⁹) and KOBr and testing its behavior when strong acid or base is added to it. Part 1 First, Lareina combines 82.86 g KOBr and 250 mL of 1.50 M HOBr, and adds enough distilled water to make 925 mL of solution. What is the pH of this solution? pH solution= Part 2 Next, Lareina adds 16.0 mL of 2.20 M HNO3 to 350 mL of the solution made in Part 1. What is the pH of the solution after the HNO, is added? pH after HNO, added = Part 3 Finally, Lareina 16.0 mL of 2.00 M NaOH ito 395 mL of the solution made in Part 1. What is the pH of the solution after the NaOH is added? pH after NaOH added =

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 188IP: Isocyanic acid (HNCO) can be prepared by heating sodium cyanate in the presence of solid oxalic acid...

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One half liter (500. mL) of 2.50 M HCl is mixed with 250. mL of 3.75 M HCl. Assuming the total solution volume after mixing is 750. mL, what is the concentration of hydrochloric acid in the resulting solution? What is its pH?
A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
. A buffered solution is prepared containing acetic acid, HC2H3O2, and sodium acetate, NaC2H3O2, both at 0.5 M. Write a chemical equation showing how this buffered solution would resist a decrease in its pH if a few drops of aqueous strong acid HCI solution were added to it. Write a chemical equation showing how this buffered solution would resist an increase in its pH if a few drops of aqueous strong base NaOH solution were added to it.
Does the pH of the solution increase, decrease, or stay the same when you (a) Add solid sodium oxalate, Na2C2O4, to 50.0 mL of 0.015-M oxalic acid? (b) Add solid ammonium chloride to 100. mL of 0.016-M HCl? (c) Add 20.0 g NaCl to 1.0 L of 0.012-M sodium acetate, NaCH3COO?
Find [OH] and the pH of the following solutions. (a) 0.25 g barium hydroxide, Ba(OH)2, dissolved in enough water to make 0.655 L of solution (b) A 3.00 L solution of KOH is prepared by diluting 300.0 mL 0.149 M KOH with water.
Two strategies are also followed when solving for the pH of a base in water. What is the strategy for calculating the pH of a strong base in water? List the strong bases mentioned in the text that should be committed to memory. Why is calculating the pH of Ca(OH)2 solutions a little more difficult than calculating the pH of NaOH solutions? Most bases are weak bases. The presence of what element most commonly results in basic properties for an organic compound? What is present on this element in compounds that allows it to accept a proton? Table 13-3 and Appendix 5 of the text list Kb values for some weak bases. What strategy is used to solve for the pH of a weak base in water? What assumptions are made when solving for the pH of weak base solutions? If the 5% rule fails, how do you calculate the pH of a weak base in water?
Consider 1.0 L of an aqueous solution that contains 0.10 M sulfuric acid to which 0.30 mole of barium nitrate is added. Assuming no change in volume of the solution, determine the pH, the concentration of barium ions in the final solution, and the mass of solid formed.
Isocyanic acid (HNCO) can be prepared by heating sodium cyanate in the presence of solid oxalic acid according to the equation 2NaOCN(s)+H2C2O4(s)2HNCO(l)+Na2C2O4(s) Upon isolating pure HNCO(l), an aqueous solution of HNCO can be prepared by dissolving the liquid HNCO in water. What is the pH of a l00.-mL solution of HNCO prepared from the reaction of 10.0 g each of NaOCN and H2C2O4, assuming all of the HNCO produced is dissolved in solution? (Ka of HNCO = 1.2 l04.)
Consider the following ions: NH4+, CO32, Br, S2, and ClO4. (a) Which of these ions in water gives an acidic solution and which gives a basic solution? (b) Which of these anions will have no effect on the pH of an aqueous solution? (c) Which ion is the strong base? (d) Write a chemical equation for the reaction of each basic anion with water.
A solution of sodium cyanide, NaCN, has a pH of 12.10. How many grams of NaCN are in 425 mL of a solution with the same pH?
Sodium bicarbonate, NaHCO3, is used in baking powder formulations and in the manufacture of plastics and ceramics, among other things. If 26.3 g of the compound is dissolved in enough water to make 200. mL of solution, what is the concentration of NaHCO3? What are the concentrations of the ions in solution?
A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution but reverses the two solutions and places the weak acid solution in the buret. After 23.75 mL of the weak acid solution has been added to 50.0 mL of the 0.100 M NaOH solution, the pH of the resulting solution is 10.50. Calculate the original concentration of the solution of weak acid.