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please show full work for understanding purposes:) 5. (4 pts) Calculate the pH of a 0.0025 M aqueous solution of s...
5. (4 pts) Calculate the pH of a 0.0025 M aqueous solution of strontium hydroxide, Sr(OH)....
5. (4 pts) Calculate the pH of a 0.0025 M aqueous solution of strontium hydroxide, Sr(OH). 5. (4 pts) Calcula pH =
Question 10 3 pts What is the pH of an aqueous 0.0025 M NaOH solution? 10,20...
Question 10 3 pts What is the pH of an aqueous 0.0025 M NaOH solution? 10,20 8.95 11.40 2.60
4. 16.55 Calculate the pH of an aqueous solution at 25°C that is 0.095 M in...
4. 16.55 Calculate the pH of an aqueous solution at 25°C that is 0.095 M in hydrocyanic acid (HCN). (K for hydrocyanic acid=4.9 x 1010 Answers TOmTzctu. 10. 16.61 Calculate the Ka of a weak acid if a 0.19-M aqueous solution of the acid has a pH of 4.52 at 25°C Answers 2. 16.71 The pH of a 0.30-M solution of a weak base is 10.66 at 25°C. What is the K of the base? Answers 4. 16.73 Calculate the...
1. 50.0 mL of a pH 6.00 carbonic acid buffer is titrated with 0.2857 M NaOH,...
1. 50.0 mL of a pH 6.00 carbonic acid buffer is titrated with 0.2857 M NaOH, requiring 17.47 mL to reach the second equivalence point. a. Calculate the molarity of carbonic acid and bicarbonate in the original buffer. (10 pts) Carbonic acid Bicarbonate: b. Calculate the pH of the solution after a total of 100.0 mL of 0.2857 M NaOH is added to the buffer and equilibrium is established. (10 pts) c. 7.833 g of solid lead(II) carbonate is added...
please show steps 16.36 Calculate the pH of an aqueous solution at 25°C that is (a)...
please show steps
16.36 Calculate the pH of an aqueous solution at 25°C that is (a) 0.12 M in HCI, (b) 2.4 M in HNO3, and (c) 3.2 X 10 M in HCIO4 16.54 Calculate the pH of an aqueous solution at 25°C that is 0.34 M in phenol (CH5OH). (K, for phenol - 1.3 x 1010 The pH of an aqueous acid solution is 6.20 at 25°C. Calculate the K, for the acid. The initial acid 16.60 concentration is...
A. Calculate the pH of a 0.0001 M HNO3 solution B. Calculate the pH of 0.08...
A. Calculate the pH of a 0.0001 M HNO3 solution B. Calculate the pH of 0.08 M Sr(OH)2 solution C. Calculate the pH of a 0.02 M hydrazoic acid solution (HN3 ----> (H+) + (N3-)), pKa = 4.72 D. Aluminum carbonate (AI2(CO3)3) reacts with phosphoric acid(H3PO4) to produce aluminum phosphate (AIPO4), carbon dioxide, and water 1. Write a balanced equation for the reaction 2. Calculate the mass of phosphoric acid (g) required to react with 100 g of an aluminum...
6. (6 pts) Calculate the pH of a 0.175 M NH3 aqueous solution. K. for NHz...
6. (6 pts) Calculate the pH of a 0.175 M NH3 aqueous solution. K. for NHz is 1.8 x 105. pH = 180
please explain how you got these answers!! and me 17) (5 pts) Calculate the pH of...
please explain how you got these answers!!
and me 17) (5 pts) Calculate the pH of a solution that is 0.15 Min ammonia (NH3) and 0.40 ammonium chloride, given the ionization constant of the base, kb, NH3 = 1.76 X 10 equilibrium reaction: NH3(aq) + H20 (1) 2 NH4(aq) + OH' (aq) A) 5.18 B) 8.82 C) 9.25 D) 9.50 E) 9.63 18) (5 pts) By far the most important buffer for maintaining acid-base balance in the blood is the...
8. (4 pts) The biological catalyst carbonic anhydrase converts carbon dioxide to carbonic acid, an essential...
8. (4 pts) The biological catalyst carbonic anhydrase converts carbon dioxide to carbonic acid, an essential component of the bicarbonate buffer system regulating our blood pH. What mass (in me) of sodium carbonate (NaHCO, MM: 84.006 g/mol) must be added to 500.0 ml of 0.029 M carbonic acid (K. 1 4.3 x 10-7, K., 4.8 x 10-11) to produce a solution with pH = 7.40? Assume no volume change after the addition of sodium carbonate. H2CO3 + H2O=HCO3 + H20...
A) Calculate the pH of a 0.0116 M aqueous solution of methylamine (CH3NH2, Kb = 4.2×10-4)...
A) Calculate the pH of a 0.0116 M aqueous solution of methylamine (CH3NH2, Kb = 4.2×10-4) and the equilibrium concentrations of the weak base and its conjugate acid. pH = ? [CH3NH2]equilibrium = ? M [CH3NH3+ ]equilibrium = ? M B)Calculate the pH of a 0.0115 M aqueous solution of nitrous acid (HNO2, Ka= 4.6×10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH = ? [HNO2]equilibrium = ? M [NO2- ]equilibrium = ? M C)...
5. (4 pts) Calculate the pH of a 0.0025 M aqueous solution of strontium hydroxide, Sr(OH). 5. (4 pts) Calcula pH =
Question 10 3 pts What is the pH of an aqueous 0.0025 M NaOH solution? 10,20 8.95 11.40 2.60
4. 16.55 Calculate the pH of an aqueous solution at 25°C that is 0.095 M in hydrocyanic acid (HCN). (K for hydrocyanic acid=4.9 x 1010 Answers TOmTzctu. 10. 16.61 Calculate the Ka of a weak acid if a 0.19-M aqueous solution of the acid has a pH of 4.52 at 25°C Answers 2. 16.71 The pH of a 0.30-M solution of a weak base is 10.66 at 25°C. What is the K of the base? Answers 4. 16.73 Calculate the...
1. 50.0 mL of a pH 6.00 carbonic acid buffer is titrated with 0.2857 M NaOH, requiring 17.47 mL to reach the second equivalence point. a. Calculate the molarity of carbonic acid and bicarbonate in the original buffer. (10 pts) Carbonic acid Bicarbonate: b. Calculate the pH of the solution after a total of 100.0 mL of 0.2857 M NaOH is added to the buffer and equilibrium is established. (10 pts) c. 7.833 g of solid lead(II) carbonate is added...
please show steps
16.36 Calculate the pH of an aqueous solution at 25°C that is (a) 0.12 M in HCI, (b) 2.4 M in HNO3, and (c) 3.2 X 10 M in HCIO4 16.54 Calculate the pH of an aqueous solution at 25°C that is 0.34 M in phenol (CH5OH). (K, for phenol - 1.3 x 1010 The pH of an aqueous acid solution is 6.20 at 25°C. Calculate the K, for the acid. The initial acid 16.60 concentration is...
6. (6 pts) Calculate the pH of a 0.175 M NH3 aqueous solution. K. for NHz is 1.8 x 105. pH = 180
please explain how you got these answers!!
and me 17) (5 pts) Calculate the pH of a solution that is 0.15 Min ammonia (NH3) and 0.40 ammonium chloride, given the ionization constant of the base, kb, NH3 = 1.76 X 10 equilibrium reaction: NH3(aq) + H20 (1) 2 NH4(aq) + OH' (aq) A) 5.18 B) 8.82 C) 9.25 D) 9.50 E) 9.63 18) (5 pts) By far the most important buffer for maintaining acid-base balance in the blood is the...
8. (4 pts) The biological catalyst carbonic anhydrase converts carbon dioxide to carbonic acid, an essential component of the bicarbonate buffer system regulating our blood pH. What mass (in me) of sodium carbonate (NaHCO, MM: 84.006 g/mol) must be added to 500.0 ml of 0.029 M carbonic acid (K. 1 4.3 x 10-7, K., 4.8 x 10-11) to produce a solution with pH = 7.40? Assume no volume change after the addition of sodium carbonate. H2CO3 + H2O=HCO3 + H20...
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