Chemistry
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ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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What is the pH of a buffer solution that is 0.20 M methyl
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- Determine the pH of a 0.275 M KOH solution. Give your answer to 2 decimal places in regular notation. Determine the pH of a 0.150 M aniline solution (Kb = 4.3x10-10). Give your answer to 2 decimal place in regular notation. Determine the pH of a 0.175 M Phenol solution (Ka = 1.3x10-10). Give your answer to 2 decimal place in regular notation.arrow_forwardCalculate the pH of a mixture containing 0.23 M HONH2 and 0.44 M HONH3Cl. (Kb = 1.1 × 10–8) What information do we need to calculate the pH? (Choose all letters that apply.) a. 0.23 M HONH2b. 0.44 M HONH3Clc. the major species in the solutiond. pOH = –log[OH–] and 14.00 = pOH + pHe. Kb = 1.1 × 10–8arrow_forward2) a) Eggshells, CaCO3, are not very soluble but they will dissolve to a small degree. Predict if solution of crushed eggshells will be acidic, basic, or neutral. Write any hydrolysis reactions that apply and use the appropriate K, and K, values to explain your prediction. Are eggshells, CaCO₂, solution = b) Potassium hydrogen phthalate, KHC,H4O4, also known as KHP, is an acidic salt. It is often used as a primary standard in acid-base titrations. It is a solid that is not hygroscopic, making it easy to weigh accurately. Write the dissociation reaction of KHC₂H₂O₂. It dissociates into ONE cation and ONE anion: HC H₂O4 is an amphoteric anion. Write the K, hydrolysis reaction for HC H₂O4™- Write the K, hydrolysis reaction for HC₂H₂O. (acidic, basic or neutral) Which is greater in value, the K, for HC₂H4O; or the K₂ for HC₂H₂O₂ ? How did you make your determination?arrow_forward
- How many milliliters of 2.5M benzoic acid need to be added to 500. mL of a solution already contains 6.00 grams of sodium benzoate, if you want the final pH to be 4.55? Ka for benzoic acid =6.28x10^-5 (B)if you add 16 grams of sodium benzoate to 4.55 grams of benzoic acid to a 1.00 liter container of water, what is the pH of this solution? (c)how many grams of potassium nitrite need to be added to 250.0 mL of a 0.1500 M HNO2 solution to produce a final buffer at pH=3.65? Ka for HNO2=4.5x10^-4arrow_forwardHelp with the following questionarrow_forwardHow to calculate the ph? What would be the result if the acid was a di or tripotic? How do the calculation for them?arrow_forward
- A solution is prepared that is initially 0.20M in hypochlorous acid (HC1O) and 0.092 Min potassium hypochlorite (KC10). Complete the reaction table below, so that you could use it to calculate the pH of this solution. Use X to stand for the unknown change in [H₂O*].· . You can leave out the M symbol for molarity. initial change final [HCIO] 0 [CIO] 0 0 [H₂0] 0 || 0 Sarrow_forwardA solid hydroxide, with the formula M(OH)3, is dissolve to make a saturated solution. If the pH of the solution is 9.22, what is the Ksp of the solid? What is the solubility of the solid in g/100mL? assume that the molar mass of M is 379.5 g/mol. (In case it isn't obvious, M is a hypothetical metal)arrow_forwardyou need to prepare a pH = 9.20 buffer solution containing NH3 and NH4Cl. if you start with 0.52 M NH4Cl solution, what concentration of NH3 will you need to start with. Kb for NH3 is 1.8x10^-5. Answer in two decimals and with units.arrow_forward
- Which of the following represent a buffer system? Match the phrases in the left column to the appropriate blanks in the sentences on the right. it is missing the salt of the weak acid it is a mixture of a strong acid and a strong base it contains only a neutral salt is not it is a salt of a strong acid and a strong base it contains a weak acid and its salt is A system with both H3 C6H5O7 and Na3 C6H5O7 is not classified as a buffer system because it is a mixture of a strong acid and a strong base A system with only HNO₂ is not classified as a buffer system because it contains only a neutral salt A system with both HBr and KOH is not classified as a buffer system because it is missing the salt of the weak acid A system with only LiC1O4 is classified as a buffer system because it contains a weak acid and its saltarrow_forwardA buffer prepared by adding 115.0 mL of 0.17 M NH3 to 145.0 mL of 0.15 M NH4NO3. What is the pH of the final solution? The Kb of NH3 is 1.8x10-5. You do not need to solve the quadratic equation for this problem. Express your answer to two decimal places.arrow_forwardDetermine the pH of a solution that is prepared by dissolving 7.2 g of Ba(OH)2 in 4.7 L water at 25°C. Assume that the volume of the solvent does not change upon addition of the solute. Atomic Weights: Ba = 137.3 g/mol; O = 16.00 g/mol; H = 1.008 g/mol. Express your answer in two decimal places only. Do not put the units.arrow_forward
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