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Concept explainers
(a)
Interpretation:
The concentrations of given species are should be determined by using given concentrations.
Concept introduction:
Concentration of ion:
The electrolyte is chemical compound, which is dissociated to produce the ions in aqueous solutions.
The concentrations of produced ions in aqueous solution are given by the multiplication of coefficient of the ion with concentration of solution.
(b)
Interpretation:
The concentrations of given species are should be determined by using given concentrations.
Concept introduction:
Concentration of ion:
The electrolyte is chemical compound, which is dissociated to produce the ions in aqueous solutions.
The concentrations of produced ions in aqueous solution are given by the multiplication of coefficient of the ion with concentration of solution.
(c)
Interpretation:
The concentrations of given species are should be determined by using given concentrations.
Concept introduction:
Concentration of ion:
The electrolyte is chemical compound, which is dissociated to produce the ions in aqueous solutions.
The concentrations of produced ions in aqueous solution are given by the multiplication of coefficient of the ion with concentration of solution.
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Chapter 9 Solutions
Chemistry: Atoms First
- The major component of vinegar is acetic acid, CH3COOH. Its Ka is 1.8 × 10-5 . One student used 1.000 M NaOH to titrate 25.00 mL vinegar. At the end point, 21.82 mL NaOH was used. (a) What is the concentration of CH3COOH in vinegar? (b) What is the pH of the solution at the end point? (c) What indicator(s) the student should use in this titration? Explainarrow_forwardThe following 4 questions involve the titration of a 50.00 mL sample of 0.200 M chlorous acid, HClO2, with 0.200 M NaOH (aq., 25 oC). The Ka HClO2 = 1.11 x 10–2 1. Calculate the pH of the solution before any NaOH has been added.arrow_forwardDetermine the hydronium ion concentration for a solution of 0.550 M Ca(OH)2.arrow_forward
- A chemistry graduate student is given 125. mL of a 0.80M ammonia (NH3) solution. Ammonia is a weak base with K₂ = 1.8 × 10. What mass of NHÂBr should the student dissolve in the NH3 solution to turn it into a buffer with pH = 9.55? 4 You may assume that the volume of the solution doesn't change when the NH Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 0 x10 × Sarrow_forward(a) A 50.0 mL solution is prepared to be 1.29 M acetylsalicylic acid. In the first step, 8.55 mL of NaOH is titrated into the solution until the pH is exactly 5.0. What is the concentration of the titrant (NaOH)? (b) In the second step, enough 5.85 M nitric acid is added to the solution after the titration in part (a) is complete until the pH is one unit lower than the pKa of acetylsalicylic acid. What volume (mL) of nitric acid was added?arrow_forwardA 50.00-mL sample of a white dinner wine required 24.57 mL of 0.03291 M NaOH to achieve a phenolphthalein end point. Express the acidity of the wine in grams of tartaric acid (H2C4H4O6; 150.09 g/mol) per 100 mL. (Assume that two hydrogens of the acid are titrated).arrow_forward
- 1. If 30.00 ml of a 0.300 mol/L of a weak acid, CH,CO,H (aq), is titrated with a 0.300 mol/L NaOH(aq), a strong base, determine the amount/moles and pH of the remaining acid after K, = 1.8 x 10* (a) 0.00 mL of NaOH is added (b) 10.00 mL of NaOH has been added. O at equivalency point when 30.00ml of NaOH was added. (d) Explain why the pH differs in (b) and (c)arrow_forwardThe acidity of a solution is measured by its pH. If HT| represents the concentration of hydrogen ions (in moles/liter) in the solution, the pH is defined by pH = – log H+ Based on careful measurements and calculations, a chemist examines two solutions and asserts: "The hydrogen ion concentration of Solution A is 37.93% greater than the hydrogen ion concentration of Solution B." If the pH of solution B is 4.36, determine the pH of Solution A. Report your answer to two decimal places. Solution A has pH equal to Number - (Report to the nearest 0.01)arrow_forwardAqueous solutions of Al3+ are acidic due to the following reaction: Al(H2O) 3+6 (aq) → Al(H2O)5OH2+ (aq) + H+(aq) If the concentrations of H+ and Al(H2O)5OH2+ are found to be (2.74x10^-3) M in a solution that was initially (1.3x10^-1) M in Al(H2O)63+, calculate the equilibrium constant for the reaction. (Hint: Make a RICE table to solve this problem). Note: Your answer is assumed to be reduced to the highest power possible.arrow_forward
- Be sure to answer all parts. Enter your answers in scientific notation. Calculate the hydronium ion concentrations of the following solutions at 25°C, given the pH. (a) pH = 9.20 %3D [H,0*]=Ox 10. (b) рH %3D 3.82 [H,0*] = x 10 Marrow_forwardRed cabbage juice is a sensitive acid-base indicator; its colors range from red at acidic pH to yellow in alkaline solutions. If red cabbage is used for the following titration, calculate the pH of the solution described and indicate whether the solution will be red or yellow. If 67.00 mL of a 1.980 M HNO2 solution is reacted with 2.350 g NaOH, calculate the resulting pH. Resulting pH = Color of Solution =arrow_forwardThe barium oxide is a strong electrolye: BaO(s) + H2O(l) → Ba2+(aq) + 2 OH−(aq). What is the pH of a solution prepared by dissolving 0.175 g of solid BaO in enough water to make 1.00 L of aqueous solution (at 25°C)? Enter your answer in decimal format with two decimal places (value ± 0.02). The answer is 11.36 would like an explanation to this problem please.arrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
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