5. Calculate the [H+] of the following mixtures
Calculate the [H+] of the following mixtures
a. Dilution and Weak Acid problem: 25 mL of 0.10 M ascorbic acid and 25 mL of water
b. Dilution and Conjugate Acid problem: 25.0 mL of 2.50 × 10-3 M nicotine (for which Kb = 1.05 × 10-6) and 50.0 mL of 1.25 × 10-3 M HCl
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5. Calculate the [H ] of the following mixtures. (2.5 marks per part) a. Dilution and...
5. Calculate the [H ] of the following mixtures. (2.5 marks per part) a. Dilution and Common lon problem: 25 mL of 0.10 M HCIO, and 25 mL of 0.15 M HCIO (K 2.9 x 10* b. Buffer problem: 25 mL of 0.025 M lactic acid (for which K of 0.015 M NaOH 1.37 x 10) and 25 mL c. Dilution and Weak Acid problem: 25 mL of 0.10 M ascorbic acid and 25 mL of water d. Dilution and...
Can anyone please help with how to calculate degree of ionization for the first 3 solutions...
Can anyone please help with how to calculate degree of
ionization for the first 3 solutions as well as how to calculate
the expected pH for solution 4? thank you!
Experiment 8: Equilibria of Weak Acids and Bases Lab Report Sheet 1 Composition 20.0 mL of 0.1 M HC2H302 - (A weak acid) pH 12.76 2.42 2.59 10.0 mL of 0.10 M HC2H3O2 + 10.0 mL H20 - (effect of dilution on the degree of ionization of weak acid) 10.0...
Calculate the final temperature for each of the following mixtures. Assume no heat loss to the...
Calculate the final temperature for each of the following mixtures. Assume no heat loss to the environment. Show your method for part b. 50.0 g of water at 25.0 degree C is mixed with 50.0 g of water at 85.0 degree C. 75.0 g of water at 25.0 degree C is mixed with 25.0 g of water at 85.0 degree C. In Part B of this experiment, 0.10 g of Mg is added to 50. mL of 1.0M HCl. Which...
3. Weak Base versus Strong Acid Derive a titration curve for the titration of 50.0 mL of 0.10 M NH3 (Kb=1.8 x 10-5) wit...
3. Weak Base versus Strong Acid Derive a titration curve for the titration of 50.0 mL of 0.10 M NH3 (Kb=1.8 x 10-5) with 0.25 M HCl. Calculate the pH for the following volumes of HCl (0 mL, 10 mL, 15 mL, 20 ml, 25 mL, 30 mL, 35 mL). Volume of HCI, in milliters 0 pH (a) 10 15 (d) 20 |(f) 25 30 35 (g) pH at the equivalence point Specify your choice of indicator
Please answer both 24 & 27 22. Calculate the pH of a 0.0120 M lactic acid...
Please answer both 24 & 27
22. Calculate the pH of a 0.0120 M lactic acid solution. HC3H5O3, K = 1.36x10 23. Find the pH of 0.388 M lithium butanoate solution, LIC,H,O,(aq). Butanoic acid Kg = 1.52x10° 24. Calculate the percent ionization for a 0.0240 M hypochlorous acid solution. The K, for hypochlorous acid is 3.4x10 25. Nicotine is a weak base (C10H24N2, Kb = 1.0x10'). A researcher prepares a solution containing 0.300 M nicotine and 0.050 M NaOH. Determine...
1. Calculate the pH at 25°C of a 0.757 M solution of a weak acid that...
1. Calculate the pH at 25°C of a 0.757 M solution of a weak acid that has Ka = 9.28 x 10 2. Determine the Kb of a weak base if a 2.50 M solution of the base has a pH of 9.595 at 25°C. 3. The overall dissociation of malonic acid, H2C3H2O4, is represented below. The overall dissociation constant is also indicated. H2C3H204 = 2 H+ + C3H2042- K = 3.0 x 10-9 To a 0.025-molar solution of malonic...
1. Calculate the equilibrium concentrations of all species present and the pH of a solution obtained...
1. Calculate the equilibrium concentrations of all species present and the pH of a solution obtained by adding 0.100 moles of solid NaOH to 1.00 L of 15.0 M NH3. Kb = 1.8 × 10–5 2. One mole of a weak acid HA was dissolved in 2.0 L of water. After the system had come to equilibrium, the concentration of HA was found to be 0.45 M. Calculate the Ka for this weak acid. 3. Calculate the pH of a...
1.Calculate the pH at the following points in the titration of 50.0 mL of 0.100 methylamine (CH,N...
1.Calculate the pH at the following points in the titration of 50.0 mL of 0.100 methylamine (CH,NH), Kb = 4.4 x 104, with a 0.200 M HCl solution before any acid is added, after adding 0.0mL, 15.0 mL, 25.0 mL, 35.0 mL and 50 mL of HCl. Plot (using graph paper) the titraticn curve from your results (label all relevant points).
1.Calculate the pH at the following points in the titration of 50.0 mL of 0.100 methylamine (CH,NH), Kb =...
4. Calculate the initial concentrations of Fe3+ and SCN? in each of the equilibrium mixtures you...
4. Calculate the initial concentrations of Fe3+ and SCN? in each of the equilibrium mixtures you will prepare using the information in Table 2 Volume of delonged water (ml) Total volume ml) Table 2. Preparation of Equilibrium Mixtures Volume of Volume of Volume of 0.10 M Mixture 0.00200 M 0.00200 M HNO, (ml) KSCN (ML) Fe(NO3)3 (ml) 1,50 3.00 1.00 2.00 1.00 2.50 1.00 1.50 350 1.00 1.00 2.50 2.00 4.50 4.50 4.50 4.50 4.50 10.00 10.00 10.00 10.00 10.00...
Calculate the pH of the following solutions: 50.0 mL 0.10 M acetic acid + 1.0 mL...
Calculate the pH of the following solutions: 50.0 mL 0.10 M acetic acid + 1.0 mL 1.0 M HCl 50.0 mL 0.10 M acetic acid + 1.0 mL 1.0 M NaOH 50.0 mL 0.10 M sodium acetate + 1.0 mL 1.0 M HCl 50.0 mL 0.10 M sodium acetate + 1.0 mL 1.0 M NaOH 50.0 mL 0.10 M acetic acid/sodium acetate buffer 50.0 mL 0.10 M acetic acid/sodium acetate buffer + 1.0 mL 1.0 M HCl 50.0 mL 0.10...
5. Calculate the [H ] of the following mixtures. (2.5 marks per part) a. Dilution and Common lon problem: 25 mL of 0.10 M HCIO, and 25 mL of 0.15 M HCIO (K 2.9 x 10* b. Buffer problem: 25 mL of 0.025 M lactic acid (for which K of 0.015 M NaOH 1.37 x 10) and 25 mL c. Dilution and Weak Acid problem: 25 mL of 0.10 M ascorbic acid and 25 mL of water d. Dilution and...
Can anyone please help with how to calculate degree of
ionization for the first 3 solutions as well as how to calculate
the expected pH for solution 4? thank you!
Experiment 8: Equilibria of Weak Acids and Bases Lab Report Sheet 1 Composition 20.0 mL of 0.1 M HC2H302 - (A weak acid) pH 12.76 2.42 2.59 10.0 mL of 0.10 M HC2H3O2 + 10.0 mL H20 - (effect of dilution on the degree of ionization of weak acid) 10.0...
Calculate the final temperature for each of the following mixtures. Assume no heat loss to the environment. Show your method for part b. 50.0 g of water at 25.0 degree C is mixed with 50.0 g of water at 85.0 degree C. 75.0 g of water at 25.0 degree C is mixed with 25.0 g of water at 85.0 degree C. In Part B of this experiment, 0.10 g of Mg is added to 50. mL of 1.0M HCl. Which...
3. Weak Base versus Strong Acid Derive a titration curve for the titration of 50.0 mL of 0.10 M NH3 (Kb=1.8 x 10-5) with 0.25 M HCl. Calculate the pH for the following volumes of HCl (0 mL, 10 mL, 15 mL, 20 ml, 25 mL, 30 mL, 35 mL). Volume of HCI, in milliters 0 pH (a) 10 15 (d) 20 |(f) 25 30 35 (g) pH at the equivalence point Specify your choice of indicator
Please answer both 24 & 27
22. Calculate the pH of a 0.0120 M lactic acid solution. HC3H5O3, K = 1.36x10 23. Find the pH of 0.388 M lithium butanoate solution, LIC,H,O,(aq). Butanoic acid Kg = 1.52x10° 24. Calculate the percent ionization for a 0.0240 M hypochlorous acid solution. The K, for hypochlorous acid is 3.4x10 25. Nicotine is a weak base (C10H24N2, Kb = 1.0x10'). A researcher prepares a solution containing 0.300 M nicotine and 0.050 M NaOH. Determine...
1. Calculate the pH at 25°C of a 0.757 M solution of a weak acid that has Ka = 9.28 x 10 2. Determine the Kb of a weak base if a 2.50 M solution of the base has a pH of 9.595 at 25°C. 3. The overall dissociation of malonic acid, H2C3H2O4, is represented below. The overall dissociation constant is also indicated. H2C3H204 = 2 H+ + C3H2042- K = 3.0 x 10-9 To a 0.025-molar solution of malonic...
1.Calculate the pH at the following points in the titration of 50.0 mL of 0.100 methylamine (CH,NH), Kb = 4.4 x 104, with a 0.200 M HCl solution before any acid is added, after adding 0.0mL, 15.0 mL, 25.0 mL, 35.0 mL and 50 mL of HCl. Plot (using graph paper) the titraticn curve from your results (label all relevant points).
1.Calculate the pH at the following points in the titration of 50.0 mL of 0.100 methylamine (CH,NH), Kb =...
4. Calculate the initial concentrations of Fe3+ and SCN? in each of the equilibrium mixtures you will prepare using the information in Table 2 Volume of delonged water (ml) Total volume ml) Table 2. Preparation of Equilibrium Mixtures Volume of Volume of Volume of 0.10 M Mixture 0.00200 M 0.00200 M HNO, (ml) KSCN (ML) Fe(NO3)3 (ml) 1,50 3.00 1.00 2.00 1.00 2.50 1.00 1.50 350 1.00 1.00 2.50 2.00 4.50 4.50 4.50 4.50 4.50 10.00 10.00 10.00 10.00 10.00...
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