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![[CH coolH} = 0.205M [CH, CooNa] = 0.115m ka = 118x105 pka a log ka = -log (18 x105) = 4.745 pH = pka tog [cHz cona] o [ctt co](http://img.homeworklib.com/questions/37d1fe20-7016-11ea-889b-a9a27abf7803.png?x-oss-process=image/resize,w_560)
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please i need help with these questions.. thanks so much
1. If acetic acid has a...
If acetic acid has a concentration of 205 t it was mixed wla solution f sodium...
If acetic acid has a concentration of 205 t it was mixed wla solution f sodium acetate at a concentration of . 15M, what would the PH be if the ka=18E-5 2. If an ammonium solution had a concentration of .45, and it was mixed w/ an ammonium Chloride solution of .29, what would the pH be if the kb = 1. 865
please i need help with these questions... thanks so much Use the References to access important...
please i need help with these questions... thanks so
much
Use the References to access important values if needed for this question. How many grams of solid ammonium chloride should be added to 1.00 L of a 0.174 M ammonia solution to prepare a buffer with a pH of 9.850 ? Breg grams ammonium chloride = 2reg 2reg Submit Answer Retry Entire Group 4 more group attempts remaining A 49.5 ml sample of a 0.302 M aqueous acetic acid solution...
A buffer containing acetic acid and sodium acetate has a pH of 5.55. The K, value...
A buffer containing acetic acid and sodium acetate has a pH of 5.55. The K, value for CH3CO,H is 1.80 x 10. What is the ratio of the concentration of CH3CO H to CH3CO,t? [CH,CO,H1 CH2C0, 1 = Calculate the pH of a solution that has an ammonium chloride concentration of 0.054 M and an ammonia concentration of 0.053 M. Kb = 1.8 x 10-5 pH = What is the pH of 0.35 M acetic acid to 1.00 L of...
For a buffer made from sodium acetate and acetic acid, the Ka of acetic acid is...
For a buffer made from sodium acetate and acetic acid, the Ka of acetic acid is 1.8E-5. What mass of sodium acetate (NaCH3CO2) must be added to 2.50 L of 0.68 M acetic acid to make a buffer solution with pH = 5.75? The answer should be in two significant figures.
please i need help with these three questions.. thanks so much Use the References to access...
please i need help with these three questions.. thanks so
much
Use the References to access important values if needed for this question. Write the precipitation reaction for barium chloride in aqueous solution: Use the pull-down menus to specify the state of each reactant and product A Is barium chloride considered soluble or not soluble ? A. Soluble B. Not soluble e Relerce lo access important values I needed for this question. A solution contains 1.40x10 - Mammonium phosphate and...
1. Calculate the pKs of acetic acid. Please write out the entire calculation. 2. Calculate the...
1. Calculate the pKs of acetic acid. Please write out the entire calculation. 2. Calculate the pH of a 0.100 M acetic acid, 0.500 M sodium acetate buffer solution. You do not need to check any simplifying approximations made. 3. Calculate the pKa of the ammonium ion. Please write out the entire calculation. 4. Calculate the pH of a 0.200 M ammonia, 0.400 M ammonium chloride buffer solution. You do not need to check any simplifying approximations made.
Part A Acetic acid has a Ka of 1.8×10−5. Three acetic acid/acetate buffer solutions, A, B, and C, were made using varyi...
Part A Acetic acid has a Ka of 1.8×10−5. Three acetic acid/acetate buffer solutions, A, B, and C, were made using varying concentrations: [acetic acid] ten times greater than [acetate], [acetate] ten times greater than [acetic acid], and [acetate]=[acetic acid]. Match each buffer to the expected pH. Drag each item to the appropriate bin. Part B How many grams of dry NH4Cl need to be added to 2.40 L of a 0.100 M solution of ammonia, NH3, to prepare a...
How can I find out the Ka value of acetic acid using the ICE table? The...
How can I find out the Ka value of acetic acid using the ICE table? The solution is made of acetic acid and sodium acetate. When mixed, acetic acid has a new concentration of 0.05 M and sodium acetate has a 0.05 M concentration. The solution has a pH of 4.45.
please i need help with these questions.. thanks so much 5. When 25mL of a 1.5E-4M...
please i need help with these questions.. thanks so much
5. When 25mL of a 1.5E-4M solution of barium chloride solution is added to 50mL of a 3.2E-6 M silver (I) nitrate solution docs a precipitate appear? Ksp= 1.8E-10 6. The max amount of silver (I) chromate that will dissolve in .156M potassium chromate is what? Ksp 9E-122
A) A buffer containing acetic acid and sodium acetate has a pH of 5.45. The Ka...
A) A buffer containing acetic acid and sodium acetate has a pH of 5.45. The Ka value for CH3CO2H is 1.80 × 10-5. What is the ratio of the concentration of CH3CO2H to CH3CO2-? [CH3CO2H]/[ CH3CO2-] = _________ B) What is the pH change when 29.6 mL of 0.117 M NaOH is added to 95.4 mL of a buffer solution consisting of 0.123 M NH3 and 0.179 M NH4Cl (Ka for ammonium ion is 5.6x10^-10.) pH change =_______
If acetic acid has a concentration of 205 t it was mixed wla solution f sodium acetate at a concentration of . 15M, what would the PH be if the ka=18E-5 2. If an ammonium solution had a concentration of .45, and it was mixed w/ an ammonium Chloride solution of .29, what would the pH be if the kb = 1. 865
please i need help with these questions... thanks so
much
Use the References to access important values if needed for this question. How many grams of solid ammonium chloride should be added to 1.00 L of a 0.174 M ammonia solution to prepare a buffer with a pH of 9.850 ? Breg grams ammonium chloride = 2reg 2reg Submit Answer Retry Entire Group 4 more group attempts remaining A 49.5 ml sample of a 0.302 M aqueous acetic acid solution...
A buffer containing acetic acid and sodium acetate has a pH of 5.55. The K, value for CH3CO,H is 1.80 x 10. What is the ratio of the concentration of CH3CO H to CH3CO,t? [CH,CO,H1 CH2C0, 1 = Calculate the pH of a solution that has an ammonium chloride concentration of 0.054 M and an ammonia concentration of 0.053 M. Kb = 1.8 x 10-5 pH = What is the pH of 0.35 M acetic acid to 1.00 L of...
please i need help with these three questions.. thanks so
much
Use the References to access important values if needed for this question. Write the precipitation reaction for barium chloride in aqueous solution: Use the pull-down menus to specify the state of each reactant and product A Is barium chloride considered soluble or not soluble ? A. Soluble B. Not soluble e Relerce lo access important values I needed for this question. A solution contains 1.40x10 - Mammonium phosphate and...
1. Calculate the pKs of acetic acid. Please write out the entire calculation. 2. Calculate the pH of a 0.100 M acetic acid, 0.500 M sodium acetate buffer solution. You do not need to check any simplifying approximations made. 3. Calculate the pKa of the ammonium ion. Please write out the entire calculation. 4. Calculate the pH of a 0.200 M ammonia, 0.400 M ammonium chloride buffer solution. You do not need to check any simplifying approximations made.
please i need help with these questions.. thanks so much
5. When 25mL of a 1.5E-4M solution of barium chloride solution is added to 50mL of a 3.2E-6 M silver (I) nitrate solution docs a precipitate appear? Ksp= 1.8E-10 6. The max amount of silver (I) chromate that will dissolve in .156M potassium chromate is what? Ksp 9E-122
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