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NiSO4 + KOH precipitate

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chemistry
A solution of .12 L of 0.160 M KOH is mixed with a solution of .3 L of 0.230 M NiSO4. the equation for this reaction is: 2KOH (aq)+NiSO4 (aq) ----->K2SO4 (aq)+Ni(OH)2 (s) .89 grams of Ni(OH)2 precipitate form I need to know the concentration remaining in the solution of: 1...

Chemistry 101
A solution of .12 L of 0.160 M KOH is mixed with a solution of .3 L of 0.230 M NiSO4. the equation for this reaction is: 2KOH (aq)+NiSO4 (aq) ----->K2SO4 (aq)+Ni(OH)2 (s) .89 grams of Ni(OH)2 precipitate form I need to know the concentration remaining in the solution of: 1...

Chemistry
When we add a large amount of etilendiamine to a solution NiSO4 a lila precipitate is observed, what is this precipitate)

Chemistry
A solution of 220mL of 0.200M Koh is mixed with a solution of 120mL of 0.240M NiSO4. 1.Determine limiting reactant? 2.Calculate the mass of precipitate formed? 3.Calculate the molarity of all ions left in the solution?

chemistry
A solution of 220mL of 0.200M Koh is mixed with a solution of 120mL of 0.240M NiSO4. 1.Determine limiting reactant? 2.Calculate the mass of precipitate formed? 3.Calculate the molarity of all ions left in the solution?

Chemistry--PLEASE HELP
A solution of 220mL of 0.200M Koh is mixed with a solution of 120mL of 0.240M NiSO4. 1.Determine limiting reactant? 2.Calculate the mass of precipitate formed? 3.Calculate the molarity of all ions left in the solution?

Chemistry
You wish to make a 0.200 M solution of NiSO4 (aq). How many grams of NiSO4 * 6H2O should you put in a 0.500 L volumetric flask? The answer is 26.3 g NiSO4 * 6H20 but I am not sure how to get there.

Chemistry
How many grams of NiSO4*6H2O are needed to prepare 200*10^2 mL of a 3.5*10^-2 M NiSO4 solution?

chemistry
What mass of NiSO4 is present in 2.00 x 102ml of 6.00% NiSO4(aq)? (The density of the solution is 1.13g/ml.)

chem
you need to make .80 M solution of NiSO4 (aq). How many grams of NiSO4 * 6H2O should you put into a .50 L volumetric flask?

Chemistry
Calculate the molarity of the following solutions: 5.0g of KOH in 4.0L of KOH solution I went from grams of KOH to moles of KOH to molarity but still got the wrong answer... 5.0g KOH X 1 mol KOH/56.108g KOH = 5.0 mol KOH/56.108=0.0891 mol KOH/4.0L and got the answer of 0.02 M ...

Chemistry
If 845mL of a 2.5x10^-5 mol/L solution of Ni(NO3)2 was mixed with 195mL of a 4.86x10^-2 mol/L solution of KOH, would precipitate form? Calculate the ion product for the potential precipitate. The Ksp of Ni(OH)2(s) is 6.0x10^-16

Chemistry 22
Determine if the reaction produces a precipitate. For a precipitate mark ‘a’ and if there is no precipitate mark ‘b’. 8. KOH(aq) + Fe(NO3)3(aq)  9. MgCl2(aq) + Na(NO3)2(aq)  10. NaBr(aq) + Ag(NO3) (aq)  11. Na3PO4(aq) + Ba(NO3) 2(aq) 

Chemistry
Use the data in this table to calculate the solubility of each sparingly soluble substance in its respective solution. (a) silver bromide in 0.066 M NaBr(aq) mol · L-1 I know how to do this one, found it to be 1.167E-11 which is correct. (b) nickel(II) hydroxide in 0.256 M ...

chemistry
A solution of 114 mL of 0.190 molecules KOH is mixed with a solution of 200 mL of 0.220 molecules NiSO4. a. write a balanced equation for the reaction that occurs. identify all phases in answer

Chemistry
A solution of 114 mL of 0.160 molecules KOH is mixed with a solution of 300 mL of 0.250 molecules NiSO4. a. write a balanced equation for the reaction that occurs. identify all phases in answer

chemistry
how many ML of each of the following solutions will provide 25.0g of KOH? A)2.50 M of KOH b)0.750 M of KOH c)5.60 M of KOH NEED HELP setting up problem!!

Chemistry
Use the info below to calculate how much it would cost you to produce 500g of NiSO4*6H2O . don't forget to include the cost of the original nickel token . Na2CO3*H2O costs $6.58/3 kg 6 M H2SO4 costs $12.65/5L 9 M HNO3 costs $10.53/2.5L Show clearly how you obtained your answer...

Chemistry
Calculate the pH for each of the following points in the titration of 50.0 mL of a 2.7 M H3PO3(aq) with 2.7 M KOH(aq). pKa1 = 1.3 and pKa2 = 6.7 a) before addition of any KOH b) after addition of 25.0 mL of KOH c) after addition of 50.0 mL of KOH d) after addition of 75.0 mL ...

chemistry
A solution of KOH is prepared by dissolving 2.00 g of KOH in water to a final volume of 250 ml of solution what volume of this solution will neutralize 20.0 ml of 0.115 mol/L sulfuric acid? amount of KOH= 2.00g(1mol of KOH/ 56.01g)= 0.357 moles concentration of KOH in water = ...

Chemistry
Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.200 M HClO(aq) with 0.200 M KOH(aq). The ionization constant for HClO can be found here. A. Before any addition of KOH B. After addition of 25.0 mL of KOH C. After 30.0 mL of KOH D. After 50.0 mL...

Chemistry
Use the data in this table to calculate the solubility of each sparingly soluble substance in its respective solution. (a) silver bromide in 0.066 M NaBr(aq) mol · L-1 I know how to do this one, found it to be 1.167E-11 which is correct. (b) nickel(II) hydroxide in 0.256 M ...

Chemistry
25.0 ml of 0.235 M NiCl2 are combined with 30.0 ml of 2.260 M KOH. How many grams of nickel hydroxide will precipitate?

AP Chemistry
A chemist mixes 200.0mL of 0.800 M Fe(NO3)3 and 300.0 mL of 0.750 M K2Cr04 and enough of either 0.400 M KOH or 0.400 M Pb(no3)2 to end up with only two spectator ions in solution. a. How much precipitate will be formed b. How many mL of KOH or Pb(No3)2 must be used c. What are...

Chemistry
Calculate the pH for each of the following points in the titration of 50.0 mL of a 2.7 M H3PO3(aq) with 2.7 M KOH(aq). (a) before addition of any KOH (b) after addition of 25.0 mL of KOH (c) after addition of 50.0 mL of KOH (d) after addition of 75.0 mL of KOH (e) after ...

chemistry
Calculate the pH for each of the following points in the titration of 50.0 mL of a 1.8 M H3PO3(aq) with 1.8 M KOH(aq). before KOH after addition of 25, 50,75,100 ml KOH

chemistry
Which of the following aqueous solutions should NOT form a precipitate with aque- ous Ba(NO3)2? 1. K3PO4 2. K2SO4 3. K2CO3 4. KOH

college chemistry
Consider the titration of a 50.0 mL sample of a 0.100 M solution of the triprotic weak acid citric acid (H3C6H5O7) with 0.100 M KOH. For citric acid, the three (3) acid dissociation constant values are ka1 = 7.40x10-3, ka2 = 1.70x10-5, and ka3 = 4.00x10-7, respectively. Given ...

Chemistry 11
calculate the mass of impure KOH needed to make up 1.20 L of 0.60 mol/L KOH(aq)? Assume the impure KOH is 84% KOH by mass and 16% water.

Chemistry
Calculate the number of milliliters of 0.782 M KOH required to precipitate all of the Mn2+ ions in 112 mL of 0.461 M Mn(NO3)2 solution as Mn(OH)2.

chemistry: please check work
How many grams of solute are contained in 64.3 mL of 0.0238M KOH? Do I convert 64.3ml to L=.0643L Multiiply .0643L and .0238M KOH=.00153 Multiply .00153 and 56.105 g/mol KOH=.0858g KOH

chem
Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.150 M HClO(aq) with 0.150 M KOH(aq). The ionization constant for HClO is 4.0*10^-8 a)before addition of any KOH b)after addition of 25.0 mL of KOH c)after addition of 40.0 mL of KOH d)after ...

chemistry
How many milliliters of 0.316 M KOH are needed to react completely with 58.0 mL of 0.297 M FeCl2 solution to precipitate Fe(OH)2? The net ionic equation is: Fe2+(aq) + 2OH-(aq) → Fe(OH)2(s)

Chemistry
Which of the following aqueous solutions should form a precipitate with aqueous Fe(NO3)3? 1. KCl 2. KNO3 3. KOH 4. K2SO4

Chemistry
Which of the following aqueous solutions should form a precipitate with aqueous Fe(NO3)3? 1. KOH 2. KCl 3. K2SO4 4. KNO3

chemistry
Which of the following aqueous solutions should form a precipitate with aqueous Fe(NO3)3? 1. KNO3 2. KCl 3. K2SO4 4. KOH

AP chemistry
which of the following aqueous solutions should not form a precipitate with aqueous ba(no3)? 1. KOH 2. K2CO3 3. K2SO4 4. K3PO4

chemistry
when 0.1M solutions of the following substances are mixed, which pair will precipitate? 1) Pb(CH3COO)2 and Mg(NO3)2 2) H2SO4 and KOH 3) ((NH4)2)CO3 and Na3PO4 4) NaOH and BaCl2 5) CaCl2 and Na2CO3

Chemistry
A 25.00-mL sample of an H2SO4 (2 and 4 are subscripted) solution of unknown concentration is titrated with a .1328 M KOH solution. A volume of 38.33 mL of KOH was required to reach the endpoint. What is the concentration of the unknown H2SO4 (again, the 2 and 4 are subscripted...

Chemistry
A 25.00-mL sample of an H2SO4 (2 and 4 are subscripted) solution of unknown concentration is titrated with a .1328 M KOH solution. A volume of 38.33 mL of KOH was required to reach the endpoint. What is the concentration of the unknown H2SO4 (again, the 2 and 4 are subscripted...

Science
a flask contain 25 ml of HNO3 solution which requires 30 ml of 0.2 M KOH to complete the reaction. calculate the concentration of KOH. HNO3+ KOH= H2O + KNO3

Chemistry
A sample of KHC2O4 weighing 0.5839 g is dissolved in 25 mL of water and an endpoint is reached when 31.99 mL of KOH has been added. Calculate the molarity of the KOH solution. KHC2O4(aq) + KOH(aq) ¨ K2C2O4(aq) + H2O(l) because the coefficents are all the same, i just ...

Chemistry
Q: 26.30mL of 0.1105 mol/L H3PO4 solution is neutralized by 139.50 mL of KOH. Calculate the mass of solid KOH required to prepare 500.0 mL of this solution. In the previous part of this question, it asked the concentration of KOH and I worked it out to be concentration of KOH ...

Chemistry
A student titrates 0.025 M KOH into 50.00 ml of a solution of unknown weak acid HA. Equivalence point is reached when 30.00 ml of the KOH has been added. After 15.00ml of the KOH has been added the pH of the mixture is 3.92. A. What is the concentration of HA ? B. What is Ka ...

Chemistry
A student titrates 0.025 M KOH into 50.00 ml of a solution of unknown weak acid HA. Equivalence point is reached when 30.00 ml of the KOH has been added. After 15.00ml of the KOH has been added the pH of the mixture is 3.92. A. What is the concentration of HA ? B. What is Ka ...

chemistry
0.5 L of a 0.30 M HCl solution is titrated with a solution of 0.6 M KOH. a)What is the pH before addition of KOH? b)What is the total number of moles of acid? c)What is the pH after addition of 125 mL of KOH solution? d)What volume of the KOH solution is required to reach the ...

Chemistry
You have 30mL of .2M HF being titrated with .15M KOH. The pka is 3.17....half way to the equivalence point you have 20mL of KOH. Find the pH when you add 40mL of KOH . Find the pH when you have 100mL of KOH added. Sol:pH = pKa + log (base / acid) = -log 3.17 + log ( .009/ .006)

Chemistry
An excess of aqueous AgNO3 reacts with 24.5 mL of 5 M K2CrO4(aq) to form a precipitate. What is the precipitate? Answer: Ag2CrO4 What mass of precipitate is formed? Answer in units of g.

Chemistry
A sample of g 0.2050 oxalic acid (4.2 H2C2O H2O) required 25.52 mL of KOH solution to complete the neutralization according to rea tion: HOOCCOOH + 2 KOH + KOOCCOOK ↔ H2O Which the concentration in mol L-1 of this KOH solution? A sample of an unknown oxalate 0.3025 g ...

chem
a.)How many moles of NaOH are required to prepare 2.00L od 0.380M solution? answer is 0.760 mole of NaOH (mole/l * 2.00L) b.)What will be the molarity of a solution if 3.50 g of KOH are dissolved in water to make 150.0 mL of solution? answer is 0.52 M KOH (gKOH/molar mass KOH=...

Chem Help
Consider a solution that contains Ag+ , Ba2+, and Pb2+ each at a concentration of .2M a) You add NaCl until the concentration of Cl- is 5.0 x 10^-3 M. A white precipitate forms. How do you determine whether that precipitate was AgCl or PbCl2? b) If you separated the ...

chemistry
An AgNO3 solution (44 mL/0.44 M) has been mixed with an NaCl solution (83 mL/1.35x 10^-2 M) a)Determine the ion product of the precipitate(potential precipitate) b) Would a precipitate be created? The Ksp of AgCl(s) proves to be 1.8 x 10^-10

chemistry
Explain how you would prepare these solutions from powdered reagents and whatever glassware you needed: a. 2.0 L of 1.5 M KOH the answer is: a. To prepare 2.0 L of 1.5 M KOH, measure out 168 g of KOH and place it into a 2 L volumetric flask. Add water to the mark. BUT HOW DID ...

chemistry
Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.150 M HClO(aq) with 0.150 M KOH(aq). The ionization constant for HClO is 4.0x10^-8. pH before the addition of any KOH? pH after the addition of 25 mL of KOH? Please show the steps to solving this...

chemistry
When calcium chloride and ammonium phosphate are mixed, an insoluble precipitate of calcium phosphate forms and falls out of solution. After careful analysis of the purified precipitate, 8.16 * 10^25 atoms of calcium are found in the solid. How many other atoms are in the ...

Chemistry
In a titration of 35 mL of 0.40 M H3PO4 with 0.30 M KOH solution, what volume (in mL) of KOH solution is needed to reach the last equivalence point (i.e., point in the titration where enough KOH has been added to neutralize all three of the acidic protons in the phosphoric acid)?

1CHEM
In a titration of 35 mL of 0.40 M H3PO4 with 0.30 M KOH solution, what volume (in mL) of KOH solution is needed to reach the last equivalence point (i.e., point in the titration where enough KOH has been added to neutralize all three of the acidic protons in the phosphoric acid)?

Chemistry
In a titration of 35 mL of 0.40 M H3PO4 with 0.30 M KOH solution, what volume (in mL) of KOH solution is needed to reach the last equivalence point (i.e., point in the titration where enough KOH has been added to neutralize all three of the acidic protons in the phosphoric acid)?

chemistry
A 50.0 mL sample of 0.50 M HBr is titrated with 0.25 M KOH. What is the pH after the addition of 60.0 mL of KOH? A) 4.1 B) 13.4 C) 1.7 D) 2.0 E) 7.7 I'm confused on the process of solving this problem. My work so far: .050L X .50 mol/1L= .025 mol HBR .060L X .25 mol/1L= .015 ...

Chemistry
How many ml of a 0.827 Molar KOH solution is required for neutralization in a titration of 35.00 ml of 0.737 Molar H2SO4? Write the equation. 2KOH + H2SO4 ==> 2H2O + K2SO4 mols H2SO4 = M x L = 0.03500 L x 0.737 M = ?? mols KOH = 2 x mols H2SO4 from the equation. mols KOH = ...

Chemistry
In a titration experiment 34.12 mL of 0.902 M KOH is reacted with H2SO4. The endpoint is reached when 50.46 mL of the acid is mixed with the base. What is the molar concentration of the acid? I'm having a hard time even starting this problem, since I don't know the formula or ...

chemistry
Sodium fluoride and lead nitrate are both soluble in water. If 1.13 g of NaF and 0.232 g of Pb(NO3)2 are dissolved in sufficient water to make 1.00 L of solution, will a precipitate form? How do you know if there should be a precipitate or not? What is the chemical formula for...

Chemistry
You have three solutions, A, B, and C, each of which are believed to be one of the following: calcium hydroxide, potassium sulfate, and sodium chloride. Combining B and C results in the formation of a precipitate, but neither solution forms a precipitate with A. Also, adding ...

Chem 27
An antacid tablet weighing 3.084 g was dissolved and diluted to 100.0 mL in a volumetric flask. A 25.00-mL aliquot was removed and treated with sufficient 8-hydroxyquinoline to precipitate all of the aluminum and magnesium. After proper collection and drying, this precipitate ...

chemistry
How many milliliters of 1.50 M \rm KOH solution are needed to provide 0.140 mol of \rm KOH

chemistry
what is the % mass/volume (%W/V)of KOH in 60ml of a solution that contains 5gn of KOH?

Chemistry
A 4.00 L solution of KOH is prepared by diuling 400.0 m 0f 0.290 M KOH with warer [OH-]=

Chemistry
what is the final volume of 1% KOH soltion prepared from a 10ml of a 20% KOH solution?

Chemistry-urgent!
What volume of 2.5% (w/v) KOH can be prepared from 125 mL of a 5.0% KOH solution?

chemistry
A 35.0 ml sample of 0.225 M HBr was titrated with 42.3 ml of KOH. What is the concentration of the KOH?

Chemistry
A 35.0 ml sample of 0.225 m HBr was titrated with 42.3 ml of KOH. What is the concentration of the KOH

Chemistry
A 80.0 mL volume of 0.25 M HBr is titrated with 0.50M KOH. Calculate the pH after addition of 40.0 mL of KOH.

Chemistry
A 80.0 mL volume of 0.25 M HBr is titrated with 0.50M KOH. Calculate the pH after addition of 40.0 mL of KOH.

chemistry
if 22.5 mL of 0.383 M HCl are required to completely neutralize 20.0 mL of KOH, what is the molarity of the KOH solution?

CHEMISTRY
Suppose that 30.0 mL of 0.20 M C6H5COO(aq) is titrated with 0.30 M KOH(aq). a) What is the initial pH of the 0.20 M C6H5COOH(aq)? b) What is the pH after the addition of 15.0 mL of 0.30 M KOH(aq)? c) What volume of 0.30 M KOH(aq) is required to reach halfway to the ...

Chemistry
A solution contains the following ions: Hg2(2+) and Fe(2+). When potassium chloride is added to the solution, a precipitate forms. The precipitate is filtered off and potassium sulfate is added to the remaining solution, producing no precipitate. When potassium carbonate is ...

Chemistry
How many milliliters of 1.40 M KOH solution are needed to provide 0.120 mol of KOH? please explain how to solve

Chemistry
If 7 mL of water is added to 3 mL of a 0.50 M KOH solution, the concentration of KOH is changed to? I am not sure how to go about doing this. Please help, thank you!!! Would I do (7)(3) / 0.50?

chem
A 25.0 mL sample of 0.723 M HClO4 is titrated with a KOH solution. The H3O+ concentration after the addition of of KOH is

Chemistry
When sulfuric acid is added to magnesium nitrate, is the resulting product soluble or insoluble in water? Does a precipitate form? I think that the product is insoluble, and no precipitate forms. Is this right? The part I'm most unsure about is whether or not a precipitate forms.

Chemistry
A solution consisting of 25.00 g Nh4Cl in 178 ml of water is titrated with 0.114M KOH. How many mL of KOH are required to reach the equivalence pt?

Analytical Chemistry
Consider the titrations of 24mL of 0.050M HClO4 with 0.100 M KOH. Find the pH at the following volumes of KOH; Vb: 0.1, 5, 10, 12.40, 12.50, 12.60, 13

Analytical Chemistry
Consider the titrations of 24mL of 0.050M HClO4 with 0.100 M KOH. Find the pH at the following volumes of KOH; Vb: 0.1, 5, 10, 12.40, 12.50, 12.60, 13 mL

Chemistry
How many mL of 5.5 M KOH are needed to prepare 300 mL of 0.2 M KOH?

Chemistry
2. 12.5 ml of 0.280M HNO3 and 5.0mL of 0.920M KOH are mixed. To make the resulting solution neutral, which of the following should be added? -1.1 mol HCl -1.69 mL of 0.650M HBr -0.55 mmol Mg(OH)2 -2.2mL of 0.50M LiOH -none of the above; already neutral -KOH is in excess by 0....

chemistry
sulfamic acid, HSO3NH2, is a strong monoprotic acid that can be used to standardize a strong base : HSO3NH2(aq)+ KOH(aq) --> KSO3NH2(aq) + H20(l) A .179g sample of HSO3NH2 required 19.4 mL of an aq soln of KOH for complete reaction. whats the molarity of KOH soln?

Chemistry
Suppose that 30.0 mL of 0.20 M C6H5COOH(aq) is titrated with 0.30 M KOH(aq). (a) What is the initial pH of the 0.20 M C6H5COOH(aq)? (b) What is the pH after the addition of 15.0 mL of 0.30 M KOH(aq)? (c) What volume of 0.30 M KOH(aq) is required to reach halfway to the ...

chem...plz help
sulfamic acid, HSO3NH2, is a strong monoprotic acid that can be used to standardize a strong base : HSO3NH2(aq)+ KOH(aq) --> KSO3NH2(aq) + H20(l) A .179g sample of HSO3NH2 required 19.4 mL of an aq soln of KOH for complete reaction. whats the molarity of KOH soln?

chem class
A 25.00-mL sample of 0.723 M HClO4 is titrated with a 0.273 M KOH solution. The H3O+ concentration after the addition of 10.0 mL of KOH is ???? M.

Chemistry
Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.230 M HClO (aq) with 0.230 M KOH (aq). The ionization constant (Ka) for HClO is 4.00 x 10^-8. (b) after addition of 25.0 mL of KOH (d) after addition of 50.0 mL of KOH

Chemistry
I’m trying to precipitate out FePO4. Following the reaction: H3PO4 + FeCl3 = FePO4(s) + 3HCl I reacted phosphoric acid to ferric chloride, and according to the reaction, there should be a precipitate. But I haven’t observed a precipitate for the last 3 hours. Is there a ...

chemistry
Titration of 25.00 mL of KOH required 200.00 mL of 0.0050 M acetic acid, CH3COOH. What is the molarity (M) of the KOH solution? Please show calcutions.

Chemistry (mole question)
Calculate the molar mass of potassium hydroxide (KOH). How many atoms would we find in a 100 mL solution of 1 µM KOH?

chem
H2S(aq) + NiSO4(aq) →

chemistry
1) Aqueous solutions of potassium sulfate and ammonium nitrate are mixed together. Which statement is correct? A) Both KNO3 and NH4SO4 precipitate from solution B) A gas is released C) NH4SO4 will precipitate from solution D) KNO3 will precipitate from solution E) No reaction ...

Chemistry
A buffer is prepared by mixing 205 mL of .452 M HCl and .500 L of .400 M sodium acetate. Ka =1.80 x 10^-5 I got the pH is 4.79 but i can't figure out the grams of KOH the problem says how many grams of KOH must be added to .500 L of the buffer to change the pH by .125 units? I...

chemistry
Consider the following reaction CaCl2(aq) + 2Ag2SO4(aq) ! CaSO4(?) + 2AgCl(?) .Which of the following statements is true? 1. Both CaSO4 and AgCl will precipitate from solution. 2. Neither CaSO4 nor AgCl will precipitate from solution. 3. CaSO4 will precipitate from solution, ...

mechanical behaviour of materials
n isotropic alloy contains 5% by volume of a precipitate of radius 10nm. Assume the primary metal is in a simple cubic arrangement. The alloy has a Young's modulus E=70GPa and a Poisson's ratio ν=0.35. If Γ=0.9J/m2 (the energy needed to cut through the precipitate lattice ...

Chem
Please help are these right? A 2.3 mole sample of nitrogen (N2), has a volume of 50.0 L and a pressure of 630 mmHg. What is the temperature of the gas? 41.5 C which I converted to Kelvin and got 231.5K Calculate the molarity (M) of the following solutions: A) 2.0 moles of ...

Chemistry
Suppose that 30.0 mL of 0.20 M C6H5COOH(aq) is titrated with 0.30 M KOH(aq). Refer to table 1 and table 2. (a) What is the initial pH of the 0.20 M C6H5COOH(aq)? Using ICE i found to be 2.46 The rest I do not know how to set up or solve... (b) What is the pH after the addition...

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