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Check out a sample textbook solutionChapter 14 Solutions
Chemistry: An Atoms First Approach
- The pH of 0.10 M CH3NH2 (methylamine) is 11.8. When the chloride salt of methylamine, CH3NH3Cl, is added to this solution, does the pH increase or decrease? Explain, using Le Chteliers principle and the common-ion effect.arrow_forwardWeak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/Aarrow_forwardAmino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?arrow_forward
- Calculate the pH of solutions that are 0.25 M formic acid and 0.40 M sodium formate. 0.50 M benzoic acid and 0.15 M sodium benzoate.arrow_forwardEstimate the pH that results when the following two solutions are mixed. a) 50 mL of 0.3 M CH3COOH and 50 mL of 0.4 M KOH b) 100 mL of 0.3 M CH3COOH and 50 mL of 0.4 M NaOH c) 150 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2 d) 200 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2arrow_forwardWhat is the pH of a buffer solution that is 0.20 M methyl amine, CH3NH2 and 0.18 M methylammonium chloride CH3NH2Cl? The Kb for CH3NH2 is 4.4x10-4. You do not need to solve the quadratic equation for this problem. Express your answer to two decimal places.arrow_forward
- 1. The ionization constant (Kb) of aniline (C6H5NH2) is 2.35 x 10^-5. If 7.285 grams of aniline is dissolved in 100.0 mL of water, what are the equilibrium concentration of all species present?2. A certain acidic vitamin is essential for all mammals since it plays a role in DNA repair and cell signaling. A 0.439M solution of this acid is found to have a pH of 2.607. Based on the table below, what most likely is the identity of thisunknown acid?arrow_forwardA solution contains 0.363 M HA (Ka = 6.74:10-46.74:10-4) and 0.677 M NaA. What is the pH of this solution? What is the pH of this solution after 0.178 mol of HCl are added to 1.00 L of this solution? What is the pH of this solution after 0.356 mol of HCl are added to 1.00 L of this solution?arrow_forwardWrite the chemical reactions whose equilibrium constants are Kp and Ką for imidazole (C,H,N,) and imidazole hydrochloride (C,H,N,H*CI¯), respectively. K, reaction: 2.865 Incorrect K, reaction: 2.323 Incorrect Calculate the pH of a solution prepared by mixing 1.60 g of imidazole with 1.60 g of imidazole hydrochloride and diluting to 100.0 mL. The pKą of imidazole hydrochloride is 6.993. 2.07 pH Incorrect Calculate the pH of the solution if 2.00 mL of 1.06 M HCIO, are added. pH = Incorrect How many milliliters of 1.06 M HCI,, should be added to 1.60 g of imidazole to give a pH of 6.993? 2.865 volume: mL. Incorrectarrow_forward
- What is the pH of a buffer solution of phenol and its conjugate base. [C6H5OH] = 0.27 M and [C6H5O]- = 0.12 M. Ka = 1.0x 10-10arrow_forwarda) Why can you not prepare a solution of pH = 8 by diluting sufficiently a 0.01 M solution of HCl with water? b) You could determine Ka for benzoic acid by measuring the pH of a 0.010 M solution of benzoic acid. Why is the graphical method used in this experiment a better way of determining Ka? c) List the measurements along with their uncertainties made in the determination of the molar mass of benzoic acid. Calculate the uncertainty in the mola r mass of benzoic acid determined by the titration.arrow_forward2. Joey was tasked to ensure that an enzyme responsible for keeping his species from extinction remains biologically active. To do so, he needs to store it in a buffer solution with a pH of 10.00. Unfortunately, only three buffer systems are available in their laboratory: Buffer System Weak Acid Component Ka Conjugate Base Salt KYA Benzoic acid, C6H5COOH 6.25 x 105 NaCH₂COO MUH Boric acid, H3BO3 5.81 x 107 NaH₂BO TWO Hydrogen cyanide, HCN 6.20 X 10-10 NaCN A. In what buffer system (KYA, MUH, or TWO) will Joey store the enzyme? In your solution sheet, show calculations and briefly explain to support your answer. B. Write the equilibrium reaction involved in the buffer system. Write your answer on your solution sheet C. Calculate the amount (in mL) of the 1.75 M stock solution (pH 7.00) of the same buffer system needed to prepare 250 mL of a 0.550 M buffer pH 7.00. After preparing the buffer, Joey decided to determine the buffer capacity of the solution by titration using 0.500 M NaOH as…arrow_forward
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