Sodium bicarbonate CANNOT be analyzed when paired with sodium hydroxide. Which of the following statement/s CORRECTLY explains this phenomenon? I. NAHCO3 is an amphoteric salt II. a mixture of NazCO3 & NAOH is formed when NaOH is in excess III. a mixture NaHCO3 & NazCO3 is formed when NaOH is in excess A Il only B) I and II (c) I and II D I only

Sodium bicarbonate CANNOT be analyzed when paired with sodium hydroxide. Which of the following statement/s CORRECTLY explains this phenomenon? I. NAHCO3 is an amphoteric salt II. a mixture of NazCO3 & NAOH is formed when NaOH is in excess III. a mixture NaHCO3 & NazCO3 is formed when NaOH is in excess A Il only B) I and II (c) I and II D I only

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 75QAP: A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this...

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A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?
1. What is [H3O+] in a 0.10 M solution of HCN at 25°C? (K, for HCN = 4.0 × 10−10) 1.6 × 10−9 M 6.3 × 10−6 M 2.0 × 10−5 M 4.0 × 10−11 M
In dilute aqueous solution HF acts as a weak acid. However, pure liquid HF (boiling point = 19.5 C) is a strong acid. In liquid HF, HNO3 acts like a base and accepts protons. The acidity of liquid HF can be increased by adding one of several inorganic fluorides that ale Lewis acids and accept F- ion (for example, BF3 or SbF5]. Write balanced chemical equations for the reaction of pure HNO3 with pure HF and of pure HF with BF3.
A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution? How would you explain buffering to this friend?
Amino 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?
What is an acidbase indicator? Define the equivalence (stoichiometric) point and the end point of a titration. Why should you choose an indicator so that the two points coincide? Do the pH values of the two points have to be within 0.01 pH unit of each other? Explain.
Metacresol purple is an indicator that changes from yellow to purple at pH 8.2. (a) What is Ka for this indicator? (b) What is its pH range? (c) What is the color of a solution with pH 9.0 and a few drops of metacresol purple?
Given the following hydrolysis constants, which of the salts has the weakest parent ACID? K₂ or K, for salt 3.3 x 10-7 5.6 x 10-10 5.6 x 10-10 5.0 x 10-6 (A) (B) (C) (D) SALT NaClO2 NH4NO3 C₂H302 C₂H5NHBr NaCN A E B 2.5 x 10-5.
Which of the following combinations would be the best to buffer the pH of a solution at approximately 9? HCl and NaCl CH3COOH and CH3COONa (Ka = 1.8*10-5) NaF and HF (Ka = 7.2*10-4) NH3 and NH4Cl (Ka = 5.6*10-10)
Why is the pH of mixture made by, mixing equal volumes of 0.2 mol L–1 HCl and 0.2 mol L–1 NaCl (340mA) pH 1, the same pH as 0.1 mol L–1 HCl pH1 (260mA)
A 1.00 liter solution contains 0.45 M ammonia and 0.35 M ammonium nitrate. If 0.17 moles of hydroiodic acid are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of hydroiodic acid.) A. The number of moles of NH, will increase. B. The number of moles of NH, will remain the same. v C. The equilibrium concentration of H;0 will increase. D. The pH will remain the same. E. The ratio of [NH3] [NH,]will remain the same.
12. Which of the following can NOT be a buffer solution? (a) CH3COOH / CH3COONA (b) HF / LiF (c) NH3 / NHẠCi (d) H2PO4 / HPO42- (e) HI / Cal2