The questions below refer to a solution of butanoic acid, CH3(CH2)2-COOH, in water. The solution was...

The questions below refer to a solution of butanoic acid, CH3(CH2)2-COOH, in water. The solution was formed by adding 1.15 g of butanoic acid to enough water to make 100 mL of solution at 298K.

1. What is the initial butanoic acid concentration in the solution in moles per liter?

2. What is the pH of this solution?

3. How many mL of a 1.095 M NaOH solution would have to be added to the butanoic acid solution in order to completely neutralize the acid?

4. What will be the pH of the solution at the equivalence point, i.e. when all of the acid has reacted with the NaOH?

Expert Solution

queen_honey_blossom answered 2 years ago

What is the IUPAC name for the compound shown below? H3C-CH2-CH2-CH2-CH(-CH2-CH2-CH3)-CH2-CH2-CH3 (The parenthesis mean it is...

What is the IUPAC name for the compound shown below? H3C-CH2-CH2-CH2-CH(-CH2-CH2-CH3)-CH2-CH2-CH3 (The parenthesis mean it is branched.)

In a 0.15M aqueous solution of butanoic acid C3H7CO2H , what is the percentage of butanoic...

In a 0.15M aqueous solution of butanoic acid C3H7CO2H , what is the percentage of butanoic acid that is dissociated? You can find some data that is useful for solving this problem in the ALEKS Data resource. Round your answer to 2 significant digits. Help PLs

A 25.00 mL sample of 0.120 M of the diprotic malonic acid, HOOC-CH2-COOH, was titrated with...

A 25.00 mL sample of 0.120 M of the diprotic malonic acid, HOOC-CH2-COOH, was titrated with 0.250 M NaOH. If the following results were obtained, calculate Ka1 and Ka2. mL NaOH added: 5.00 6.00 10.00 12.00 15.00 18.00 20.00 24.00 pH: 2.68 2.83 3.53 4.26 5.21 5.69 6.00 9.24

Consider the titration of 50.0 mL of a 0.0200 M solution of butanoic acid with 0.100...

Consider the titration of 50.0 mL of a 0.0200 M solution of butanoic acid with 0.100 M NaOH. First, calculate the equivalence point (Ve). Then, calculate the pH at the following points along the titration curve. Assume fractions are exact numbers and ignore activities for all calculations in this problem. A) VNaOH= 0.000 mL B) VNaOH= 1/2Ve C) VNaOH= 4/5Ve D) VNaOH= Ve E) VNaOH= 3/2Ve

Find the pH of a 30.0 ml butanoic acid ( HA) solution ( 0.600 M )...

Find the pH of a 30.0 ml butanoic acid ( HA) solution ( 0.600 M ) when you add the following volume of 0.600 M NaOH ( 5 points ). Ka of HA = 1.5 x 10-5 (a) 0.0 ml (b) 10.0 ml (c) 15.0 ml (d) 30.0 ml (e) 50.0 ml

Which of the molecules below is the strongest base? CH3O- (CH2)2N- Cl- HO- (CH3)2NH

If 5.2 g of butanoic acid, C4H8O2, is dissolved in enough water to make 1.0 L...

If 5.2 g of butanoic acid, C4H8O2, is dissolved in enough water to make 1.0 L of solution, what is the resulting pH? Assuming complete dissociation, what is the pH of a 4.41 mg/L Ba(OH)2 solution? The Kb for an amine is 9.747 × 10-5. What percentage of the amine is protonated if the pH of a solution of the amine is 9.825? (Assume that all OH– came from the reaction of B with H2O.)

Calculate the pH of a solution starting with 200.0 mL of 0.010 M butanoic acid (pKa...

Calculate the pH of a solution starting with 200.0 mL of 0.010 M butanoic acid (pKa = 4.818) solution that has been titrated to the equivalence point with 0.050 M NaOH. Ignore activities and state your answer with 3 sig. figs. Use approximations if you can.

75mL of a 0.111 mol L-1 solution of butanoic acid(H3CCH2CH2C(=O)OH), and 38 mL of a solution...

75mL of a 0.111 mol L-1 solution of butanoic acid(H3CCH2CH2C(=O)OH), and 38 mL of a solution of KOH of molarity 0.101 mol L-1 are mixed in a 250 mL beaker. What would be the resulting solution's pH?

A chemist titrates 210.0 mL of a 0.7560 M butanoic acid (HC3H7CO2) solution with 0.6335 M...

A chemist titrates 210.0 mL of a 0.7560 M butanoic acid (HC3H7CO2) solution with 0.6335 M KOH solution at 25 degrees celsius. Calculate the pH at equivalence. The pKa of butanoic acid is 4.82. Round your answer to 2 decimal places please

Question