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3. (3 points) An aqueous solution is prepared by mixing hydrazoic acid (HN3) and NaNg and...
26. -10.1 points 0/4 Submissions Used A buffer solution contains 0.10 mol of hydrazoic acid (HN3)...
26. -10.1 points 0/4 Submissions Used A buffer solution contains 0.10 mol of hydrazoic acid (HN3) and 0.43 mol of sodium hydrazoate (NaN3) in 1.70 L. The Ka of hydrazoic acid (HN3) is ka = 1.92-05. (a) What is the pH of this buffer? pH = (b) What is the pH of the buffer after the addition of 0.05 mol of NaOH? (assume no volume change) pH = (c) What is the pH of the original buffer after the addition...
A solution is prepared by combining 3.227g of HN, (hydrazoic acid) with 1.442g of hydrazine (N.Н....
A solution is prepared by combining 3.227g of HN, (hydrazoic acid) with 1.442g of hydrazine (N.Н.) in 1 50mL of water at 25°C. The addition of the solids to the water did not cause a significant volume change. Calculate the equilibrium concentrations of HN,, N,H, N,, and N,H at 25°C Calculate the pH of the solution at 25°C (the bulk of the points comes from this part)
A solution is prepared by combining 3.227g of HN, (hydrazoic acid) with 1.442g...
In aqueous solution, the azide ion, N3−, is a weak base that accepts a proton from...
In aqueous solution, the azide ion, N3−, is a weak base that accepts a proton from water to form the hydroxide ion, OH −, and hydrazoic acid, HN3, according to the following equation. N3−(aq) + H2O(l) equilibrium reaction arrow OH −(aq) + HN3(aq) The base-dissociation constant (Kb) for this base is 4.04 ✕ 10−10. If a 0.082 M solution of azide ions is prepared, what is the final pH of the solution? (Assume that the temperature is 25°C.)
What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine,...
What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine, CH3NH2, with 25.00 mL of 0.10 M methylammonium chloride, CH3NH3C1? Assume that the volume of the solutions are additive and that Kb = 3.70 times 10-4 for methylamine. 10.27 10.57 10.87 11.78 Which statement about buffers is true? Buffers have a pH = 7. Buffers consist of a strong acid and its conjugate base. A buffer does not change pH on addition of a...
A buffer solution is prepared by mixing 1000mL of 2 0M lacthtc acid with 100.0mL of...
A buffer solution is prepared by mixing 1000mL of 2 0M lacthtc acid with 100.0mL of 20M sodium lactate. This butferis then diluted 1-5 by adding 4ooml of the buffer to 160.0mL of delonized water. the buffer to 160.0mb of deionized water Calculate the volume (in mL) of 2.oM HCI required to change pH of 50.0ml. of this diluted buffer by one pH unit. Ka (lactic acid) 1.38x104
15) The pH of a 0.63 M aqueous solution of hypobromous acid, HBrO, at 25°C is...
15) The pH of a 0.63 M aqueous solution of hypobromous acid, HBrO, at 25°C is 4.17. What is the value of K for HBro? a) 2.0 x 10 b) 1.1 x 10 c) 1.08 x 10° d) 7.34 x 10 e) 6.8 x 10 16) The molar concentration of hydronium ion in pure water at 25°C is (á) 1.0 x 10? b) 0.00 c) 1.0 x 1024 d) 1.0 e) 7.00 117) A solution is prepared by dissolving 0.23...
Consider the titration of 30.0 mL of 0.20 M nitrous acid by adding 0.0500 M aqueous...
Consider the titration of 30.0 mL of 0.20 M nitrous acid by adding 0.0500 M aqueous ammonia to it. The pH at the equivalence point is _____. (Note: This is the titration of a weak acid with a weak base.) (a) greater than 7 (b) equal to 7 (c) less than 7 (d) cannot be determined without more data (not including Ka and Kb) (e) is impossible to predict
13) A 0.0035 M aqueous solution of a particular compound has pOH 11.54. The compound is...
13) A 0.0035 M aqueous solution of a particular compound has pOH 11.54. The compound is a) a weak base b) a weak acid c) a strong base a strong acid e) a salt 14) In basic solution, a) [H30'> [OH] b) [H30 ]- [OH1 [Hs0)< [OH] d) (OH]<7.00 e) [OH] =OM 15) The pH of a 0.63 M aqueous solution of hypobromous acid, HBro, at 25°C is 4.17. What is the value of K for HBro? a2.0 x 10...
3. One liter of buffer solution was prepared by mixing 0.1 mole of acetic acid CH3COOH...
3. One liter of buffer solution was prepared by mixing 0.1 mole of acetic acid CH3COOH and 0.05 mole of sodium acetate CH3COONa. Calculate a. pH of that solution b. How much of a strong base, say NaOH, in mol/L needs to be added to that solution to change its pH to 6.0? Notes and useful data: For acetic acid pK4.75 For carbonic acid pKa 6.3 and pKa 10.3 Sodium acetate CH3COONa dissociates entirely to Na'CH3COO
(3 points) A 0.0730 M solution of a monoprotic acid is 1.07% ionized. What is the...
(3 points) A 0.0730 M solution of a monoprotic acid is 1.07% ionized. What is the pH of the solution? Calculate the Ka of the acid. (2 points) The pH of a 0.025 M solution of a monoprotic acid is 3.21. What is the Ka value for the acid? (2 points) Determine the percent ionization of a 0.0028 M HA solution. (Ka of HA = 1.4 x 10-9) (4 points) Lysine is triprotic amino acid (separately loses three H’s in...
26. -10.1 points 0/4 Submissions Used A buffer solution contains 0.10 mol of hydrazoic acid (HN3) and 0.43 mol of sodium hydrazoate (NaN3) in 1.70 L. The Ka of hydrazoic acid (HN3) is ka = 1.92-05. (a) What is the pH of this buffer? pH = (b) What is the pH of the buffer after the addition of 0.05 mol of NaOH? (assume no volume change) pH = (c) What is the pH of the original buffer after the addition...
A solution is prepared by combining 3.227g of HN, (hydrazoic acid) with 1.442g of hydrazine (N.Н.) in 1 50mL of water at 25°C. The addition of the solids to the water did not cause a significant volume change. Calculate the equilibrium concentrations of HN,, N,H, N,, and N,H at 25°C Calculate the pH of the solution at 25°C (the bulk of the points comes from this part)
A solution is prepared by combining 3.227g of HN, (hydrazoic acid) with 1.442g...
What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine, CH3NH2, with 25.00 mL of 0.10 M methylammonium chloride, CH3NH3C1? Assume that the volume of the solutions are additive and that Kb = 3.70 times 10-4 for methylamine. 10.27 10.57 10.87 11.78 Which statement about buffers is true? Buffers have a pH = 7. Buffers consist of a strong acid and its conjugate base. A buffer does not change pH on addition of a...
A buffer solution is prepared by mixing 1000mL of 2 0M lacthtc acid with 100.0mL of 20M sodium lactate. This butferis then diluted 1-5 by adding 4ooml of the buffer to 160.0mL of delonized water. the buffer to 160.0mb of deionized water Calculate the volume (in mL) of 2.oM HCI required to change pH of 50.0ml. of this diluted buffer by one pH unit. Ka (lactic acid) 1.38x104
15) The pH of a 0.63 M aqueous solution of hypobromous acid, HBrO, at 25°C is 4.17. What is the value of K for HBro? a) 2.0 x 10 b) 1.1 x 10 c) 1.08 x 10° d) 7.34 x 10 e) 6.8 x 10 16) The molar concentration of hydronium ion in pure water at 25°C is (á) 1.0 x 10? b) 0.00 c) 1.0 x 1024 d) 1.0 e) 7.00 117) A solution is prepared by dissolving 0.23...
13) A 0.0035 M aqueous solution of a particular compound has pOH 11.54. The compound is a) a weak base b) a weak acid c) a strong base a strong acid e) a salt 14) In basic solution, a) [H30'> [OH] b) [H30 ]- [OH1 [Hs0)< [OH] d) (OH]<7.00 e) [OH] =OM 15) The pH of a 0.63 M aqueous solution of hypobromous acid, HBro, at 25°C is 4.17. What is the value of K for HBro? a2.0 x 10...
3. One liter of buffer solution was prepared by mixing 0.1 mole of acetic acid CH3COOH and 0.05 mole of sodium acetate CH3COONa. Calculate a. pH of that solution b. How much of a strong base, say NaOH, in mol/L needs to be added to that solution to change its pH to 6.0? Notes and useful data: For acetic acid pK4.75 For carbonic acid pKa 6.3 and pKa 10.3 Sodium acetate CH3COONa dissociates entirely to Na'CH3COO
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