How do you calculate the molarity of 40 mL of 0.1M acetic acid (HC2H3O2) solution if...

How do you calculate the molarity of 40 mL of 0.1M acetic acid (HC2H3O2) solution if 12.76 mL 0.35 NaOH was added to reach the equivalence point?

Expert Solution

moles of acetic acid = 0.1 x 40 / 1000 = 4 x 10^-3

moles of NaOH = 0.35 x 12.76 / 1000= 4.5 x 10^-3

CH3COOH + NaOH -----------------------> CH3COONa + H2O

4 x10^-3 4.5 x 10^-3 0 0------------------> initial

0 0.5 x 10^-3 4 x 10^-3 4 x 10^-3---------------> equivalence point

in the solution NaOH remained.

moles of remained solution = 0.5 x 10^-3

molarity of solution = moles / total volume

= 0.5 x 10^-3 / 40 +12.76

= 9.47 x10^-6

molarity of solution = 9.47 x10^-6 M

queen_honey_blossom answered 1 year ago

you add 1 ml of 0.1M HCl to a solution containing 10ml of 0.2M acetic acid...

you add 1 ml of 0.1M HCl to a solution containing 10ml of 0.2M acetic acid (Ka = 1.8x10-5) and 10ml of 0.2 M sodium acetate. What is the resulting pH?

If we want to prepare 150 mL of Acetic acid (C2H4O2) solution with the molarity of...

If we want to prepare 150 mL of Acetic acid (C2H4O2) solution with the molarity of 0.20 M. How many grams of acetic acid do we need?

Calculate the pH of a 0.100M NaCH3COO solution. Ka for acetic acid, HC2H3O2 is 1.8x10-5

If you started with an acetic acid solution of 2.0 mL of 0.84M Acetic acid and...

If you started with an acetic acid solution of 2.0 mL of 0.84M Acetic acid and shifted it with 0.2mL of 0.01M HCl (4 drops), what is the new pH?. Initial pH Final pH Ka of acetic acid = 1.8 x 10-50.3 Start by finding the equilibrium concentrations of the acetic acid solution. Calculate the Ph based on this initial concentration (initial Ph). Calculate the moles of everything (compounds in the equilibrium AND the acid). Shift the equilibrium with the...

50.0 mL of a 0.1M fluoride solution is titrated with 0.1M calcium. Calculate the pCa at...

50.0 mL of a 0.1M fluoride solution is titrated with 0.1M calcium. Calculate the pCa at the halfway point in the titration.

Calculate the molarity of a solution made by adding 25.4 mL of concentrated hydrochloric acid (37.3...

Calculate the molarity of a solution made by adding 25.4 mL of concentrated hydrochloric acid (37.3 % by mass, density 1.19 g/mL) to some water in a volumetric flask, then adding water to the mark to make exactly 500 mL of solution. (It is important to add concentrated acid or base to water, rather than the other way, to minimize splashing and maximize safety.)

Calculate the molarity of a solution made by adding 39.2 mL of concentrated perchloric acid (70.5...

Calculate the molarity of a solution made by adding 39.2 mL of concentrated perchloric acid (70.5 % by mass, density 1.67 g/mL) to some water in a volumetric flask, then adding water to the mark to make exactly 2000 mL of solution. (It is important to add concentrated acid or base to water, rather than the other way, to minimize splashing and maximize safety.) [ HClO4]= _____M

A volume of 25.0mL of a 0.10M aqueous solution of acetic acid(HC2H3O2 or HOAc or CH3CO2H,...

A volume of 25.0mL of a 0.10M aqueous solution of acetic acid(HC2H3O2 or HOAc or CH3CO2H, Ka=1.8x10-5) is titrated with 0.080M NaOH. What is the pH Initially After 10.0mL of NaOH has been added At the halfway point After 20.0mL of NaOH has been added At the equivalence point And after 40.0mL NaOH has been added

Calculate the molarity of an HCl solution if a volume of 39.54 mL of this solution...

Calculate the molarity of an HCl solution if a volume of 39.54 mL of this solution is required to titrate 0.2348 g Na2CO3. (Bromocresol green is used as an indicator). This HCl solution (calculated in question 1.) is then used to analyze an unknown sample. Calculate the % Na2CO3 in the sample if a volume of 23.44 mL of the HCl solution is required to titrate 0.4089 g of the sample

Calculate the pH of a buffer solution prepared by mixing 20 mL of 5.0% acetic acid...

Calculate the pH of a buffer solution prepared by mixing 20 mL of 5.0% acetic acid with 20 mL of 0.50 M NaOH and 100 mL of water

Question