Please help me figure out how to solve a problem like this: Using initial conjugate acid and conjugate base concentrations of 0.100 M Benzoic Acid (C6H5COOH), show that the pH calculated using a Ka expression is the same as the pH calculated using a kB expression.
Please help me figure out how to solve a problem like this: Using initial conjugate acid...
Calculate the pH of each of the following aqueous solutions at 25 °C. (Please help me solve #4 with your work, and check my answers for #1-3, if incorrect please show me why, Thank you) 1) 0.65 M boric acid (B(OH)3, Ka = 7.3 x 10-10) (pH=4.66) 2) 3.15 M ammonia (NH3, Kb = 1.76 x 10-5) (pH= 4.37) 3) 0.82 M benzoic acid (C6H5COOH, Ka = 6.3 x 10-5) (pH=2.14) 4) 0.100 M H3AsO4 (Ka1 = 2.5 x 10-4,...
2. A buffer is prepared by partially titrating 50.00 mL of 0.964 M benzoic acid using 0.100 M NaOH until the pH is 4.80. Ka for benzoic acid is 6.3 x 10-5. (o)ce pts) What ratio of the conjugaite base-to-conjugate acid i equrd to establish p 4 (b) (1 pts) What volume of the titrant is required to achieve pH 4.80? (c) (2 pts) What are the final concentrations of the conjugate acid and conjugate base? 2. A buffer is...
can someone please help me? Calculate the Kb of Sodium Nitrite, NaNO2. It is the conjugate of Nitrous Acid. Show the reaction of the base Pyridine (see bottom chart) with water. 3. What is the pH of a 0.15 M solution of the base Ethylamine? 4. What is the pH of a 0.15M monoprotic acid, HA, that is 1.25% ionized?
please help with remaining questions. not sure how to figure these out or if there is more information required to figure them out. also, are the ones i have answered correct? thanks so much for your help. Caleb Davis Pre-lab Q's a. You will be titrating an acetate buffer with HCl. What is the acid and conjugate base of this buffer? HCI + CH;COO = CH3COOH + C1 (CH3COOH = conjugate acid) (conjugate base -CH2COO) b. At the half equivalence...
I can't figure this problem out. Please help! Chloroacetic acid, HC2H202CI, is a stronger monoprotic acid than acetic acid. In a 0.10 M solution, the pH is 1.96. Incorrect. Did you use the correct equilibrium expression? Did you use the correct number of significant figures? Calculate the Ka for chloroacetic acid 0.0013 Ka
Acid/Base Review Questions: 1. HIO is a weak acid with Ka = 2.00 x 10-11. a. Write the formula for the conjugate base. b. Show the reaction for the acid in water. c. Show the reaction for the conjugate base in water. d. Write the K, expression. e. Write the Kb expression. f. Write the product of Ka x Kb. g. Find the pH of the following solutions: i. 0.100 M HIO 0.115 M NaIO Buffer that is 0.100 M...
Close Proble Tutored Practice Problem 16.4.3 COUNIS TOW Calculate the pH of a weak acid solution (HAJo >100 Ka) Calculate the pH of a 0.467 M aqueous solution of hypochlorous acid (HCIo, K, 3.5 10 weak acid and its conjugate base. and the equilbrium concentrations of the pH [FICIO!equilibrium CIoaquliborium Show Approach It is not always possible to simplify the K, expression by assuming that r is small when compared to the initial acid concentration. In these cases, the weak...
1. Write the equilibrium expression for the autoionization of water. Using this expression define the terms acid and base and pH. 2. Calculate the pH, pOH, Ka, Kb, pKa, and pKb for a 0.082M solution of triethylamine. 3. Calculate the pH, pOH, Ka, Kb, pKa, and pKb for a 1.570 M solution of hydrogen cyanide. 4. The acid-dissociation constant for hypochlorus acid is 3.0 X 10-8. Calculate the concentrations of H3O+, CIO-, and HCIO at equilibrium if the initial concentration...
A buffer is prepared by partially titrating 50.00 mL of 0.964 M benzoic acid using 0,100 M NaOH until the pH is 5.80. Ka for benzoic acid is 6.3 x 10-5. a) what ratio of the conjugate base to conjugate acid is required to establish pH 4.80? b) what volume of the titrant is needed to achieve pH 4.80? c) what are the final concentrations of the conjugate acid and conjugate base?
Hey! Can you please help me with the following two questions I am highly confused and I don't really understand them at all. Thank you!! 16, Please help me with them, we have a test this thursday and problems that are similar are supposed to be on there. Thank you so much!!! 1.Calculate the pH of a 0.119 M aqueous solution of hydroxylamine (NH2OH, Kb = 9.1×10-9) and the equilibrium concentrations of the weak base and its conjugate acid. pH...