11) What would be the pH of 100.0 mL of a solution that is 0.040 M CH3COOH and 0.010 M CH3COO–? a. 5.36 b. 7.00 c. 4.16 d. Not enough information is given.
pH = pKa + log [CH3COO-] / [CH3COOH]
pKa of CH3COOH = 4.75 (standard value)
pH = 4.75 + log [0.01] / [0.04]
pH = 4.14
answer = option c = 4.16 (closest value)
11) What would be the pH of 100.0 mL of a solution that is 0.040 M...
Calculate the pH of a solution formed by mixing 100.0 mL of 0.100 M NaF and 100.0 mL of 0.040 M HCI. Ka of HF = 7.24 x 10-4. A 3.32 B.3.54 C.3.14 D.2.74 E 2.96
5. Calculate the grams of NaCH3COO required for 100.0 mL of 0.20 M CH3COOH solution to achieve a pH of 4.40. (Assume no volume change.) K = 1.8 x 10-5 6. What is the pH of 100.0 mL of buffer consisting of 0.20 M CH3COOH/0.20 M NaCH3COO after 10.0 mL of 0.20 M HC1 was added into the solution ? Kg = 1.8 x 10-5 7. The pH of a sodium acetate-acetic acid buffer is 4.80. Calculate the ratio of...
consider 100.0 ml of a buffer solution that contains [NaCH3COO]=[CH3COOH]=0.250 M a) what is the pH of this buffer? b) what should the ph of the buffer be after 50.0ml of water is added? explain c) wtite balanced net ionic for the reaction that occurs whrn 1.0 M HCl ir added to this buffer. d) after adding 10.0 ml of 1.0 M HCl what will the ph of the solution be? e) as more 1.0 M HCl is slowly added...
Calculate the pH of a solution containing the following compounds. (Note that these are concentrations before any reaction occurs). [CH3COOH] 0.040 M [CH3COO-1] 0.010 M [KOH] 0.002 M
1) Calculate the pH of the 1L buffer composed of 500 mL of 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of HCl is added (Ka HC2H3O2 = 1.75 x 10-5). Report your answer to the hundredths place. 2) Calculate the pH of the 1L buffer composed of 500 mL 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of NaOH is added (Ka HC2H3O2 = 1.75...
Calculate the pH of a solution when 100.0 mL of a 0.100 M solution of acetic acid (CH3COOH), which has a Ka value of 1.8 × 10–5, is titrated with 110 mLs of a 0.10 M NaOH solution.
11) (5 points) Calculate the pH of 100.0 mL of a 0.500 M solution of methylamin when it is titrated with 0.250 M HCl. Methylamine has a pKb of 3.36 a) 0 mL HCl added c) Equivalence point d) 10 mL past the equivalence point
If I mixed 100.0 mL of a nitric acid solution of pH = 2.40 with 100.0 mL of a nitric acid solution of pH = 2.70, what would be the pH of the mixture? Write your answer to 2 digits beyond the decimal (e.g., 8.63) If 5.15 grams of iron(III) nitrate (molar mass = 241.86 g/mol) is dissolved in enough water to prepare exactly 150.0 mL of solution, what would be the molar concentration of the nitrate ion? 0.284 M...
If 100. mL of 0.040 M NaOH solution is added to 100. mL of solution which is 0.10 M in and 0.10 M in, what be will the pH of the new solution? a. 5.00 b. 4.74 c. 4.81 d. 4.89 e. 5.11 What concentration of Al^3+ must be added to a solution of pH = 4.80 in order to initiate precipitation of Al(OH)_3 at 25 degree C? K_ for Al(OH)_3 = 1.9 times 10^- a. 5.3 times 10^-7 M...
Calculate the pH of a solution made by mixing 100.0 mL of 0.355 M NH3 with 100.0 mL of 0.100 M HCl. (Kb for NH3 = 1.8 10–5) Select one: a. 9.66 b. 8.85 c. 4.34 d. 9.26