which of the following acids should be used to prepare a buffer with ph 9.3? A.HbrO...
Which of the following acids should be used to prepare a buffer with a pH of 5.9? HOCH2COOH, Ka = 3.5 × 10–4 HClO2, Ka = 1.1 × 10–2 HBrO, Ka = 2.3 × 10–9 ClCH2COOH, Ka = 1.4 × 10–3 C6H13NO4S, Ka = 7.08 x 10-7
Which of the following weak acids could be used to prepare a buffer solution for a pH of 3.15? A. hydrofluoric acid; Ka = 3.0 x 10-7 B. hypochlorous acid; ka = 3.0 x 10-8 C. acetic acid ; Ka = 1.8x10-5 D.nitrous acid; Ka = 4.5 x 10-4
Question 1 2 pts Which of the following acids should be used to prepare a buffer with a pH of 9.3? OHBrO, K; -2.3 x 100 OCH,CO2H, K, - 1.8 10-5 HCO,H, K, - 1.7 x 104 O HCN, K, = 4,9 x 10:10
which of the following acid should be used to prepare a buffer with a pH of 9.0? Which of the following acids should be used to prepare a buffer with a pH of 9.0? A. CH3COZH, K, = 1.8 x 10-5 B. H2CO3, K4 = 4.3 x 10-7 C. HF, K, = 6.6 x 10-4 D. HCIO, K, = 3.0 x 10- E.HCN, kg = 6.2 x 10-10
A buffer is required to maintain solution pH around 3.5. a) Which of the following weak acids would selected for this buffer? Formic acid Ka: 1.8x10^-4 Benzoic acid Ka: 6.5x10^-5 Acetic acid Ka: 1.8x10^-5 How would you prepare 1.0 L of the buffer with an overall concentration of 0.750 M?
QUESTION 19 Which of the following acids should be used to prepare a buffer with a pH of 5.9? HOCH2COOH, Ka = 3.5 x 10-4 CICH2COOH, Ka = 1.4 x 10-3 HBrO, Ka = 2.3 x 10-9 C6H13NO4S, Kg = 7.08 x 10-7 HCIO2, Ka = 1.1 x 10-2 QUESTION 20 For the following reaction, N2 (9) + 1/2O2 (g) → N20 (9) At 298 K, AS surr = - 275.34 J/K and ASsys = -74.3 J/K. Which of the...
Which of the following bases should be used to prepare a buffer with a pH of 6.0? hydroxylamine, Kb = 1.1 × 10-8 ammonia, Kb = 1.8 × 10-5 pyridine, Kb = 1.7 × 10-9 anyline, Kb = 3.8 × 10-10 codeine, Kb = 1.6 × 10-6
1. To prepare a buffer solution with a pH of 3.7. Which of the following conjugated pairs would be the best option? A. HSO4- / SO42- Ka = 1.2 x10-2 B. HCN / CN- Ka = 4.0 x 10-10 C. HCHO2 / CHO2- Ka = 1.8 x 10-4 D. H2CO3 / HCO3 Ka = 4.2 x 10-7 E. HClO / ClO- Ka = 2.9 x 10-8
You work in a chemistry lab, and are asked to prepare 500 mL of a buffer solution with pH-3.20, The weak acid solution concentration in this buffer should be 0.250 M and salt is a solid. The following steps walk you through a step by step process of this preparation. a. Choose the proper weak acids for the buffer solution Table 1. Ionization constant Ka for some weak acids Name Hydrofluoric acid Nitrous acid Fulminic acid Acetic acid Hypochlorous acid...
Calculate the pH of the following solution (Ka HCO2H is 1.8x10-4 and Kb NH3 is 1.8x10-5): 0.10 M HCO2H / 0.10M NaHCO2 buffer