An analytical chemist is titrating 178.3mL of a 0.3400M solution of acetic acid HCH3CO2 with a...

An analytical chemist is titrating 178.3mL of a 0.3400M solution of acetic acid HCH3CO2 with a 0.2300M solution of NaOH . The pKa of acetic acid is 4.70 . Calculate the pH of the acid solution after the chemist has added 46.70mL of the NaOH solution to it

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queen_honey_blossom answered 1 year ago

An analytical chemist is titrating 60.5mL of a 0.8700M solution of benzoic acid HC6H5CO2 with a...

An analytical chemist is titrating 60.5mL of a 0.8700M solution of benzoic acid HC6H5CO2 with a 0.3600M solution of KOH . The pKa of benzoic acid is 4.20 . Calculate the pH of the acid solution after the chemist has added 172.mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places.

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An analytical chemist is titrating 114.8mL of a 0.3100M solution of nitrous acid HNO2 with a 1.000M solution of KOH . The pKa of nitrous acid is 3.35 . Calculate the pH of the acid solution after the chemist has added 12.69mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places.

An analytical chemist is titrating 227.3mL of a 1.200M solution of propionic acid HC2H5CO2 with a...

An analytical chemist is titrating 227.3mL of a 1.200M solution of propionic acid HC2H5CO2 with a 0.5600M solution of NaOH . The pKa of propionic acid is 4.89 . Calculate the pH of the acid solution after the chemist has added 532.8mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places.

An analytical chemist is titrating 60.3 mL of a 0.5500 M solution of nitrous acid (HNO2)...

An analytical chemist is titrating 60.3 mL of a 0.5500 M solution of nitrous acid (HNO2) with a 0.6400 M solution of KOH. The pKa of nitrous acid is 3.35. Calculate the pH of the acid solution after the chemist has added 22.2 mL of the KOH solution to it. Please round your answer to 2 decimal places

Suppose you are titrating vinegar, which is an acetic acid solution of unknown strength, with a...

Suppose you are titrating vinegar, which is an acetic acid solution of unknown strength, with a sodium hydroxide solution according to the equation H C 2 H 3 O 2 + N a O H ⟶ H 2 O + N a C 2 H 3 O 2 H C 2 H 3 O 2 + N a O H ⟶ H 2 O + N a C 2 H 3 O 2 If you require 33.38 mL of 0.1936...

a.) Write a balance equation for the dissociation of acetic acid ( HCH3CO2) in water, include...

a.) Write a balance equation for the dissociation of acetic acid ( HCH3CO2) in water, include state symbols, charges and label every reactant and product as Acid or Base. b.) If acetic acid has a Ka = 1.8 x 10-5 exponent, what is the pH of a buffer solution that contains 0.100 M acetic acid and 0.120 M sodium acetic. c.) Write the equation for the reactuon if HNO3 is added to this buffer, include all state symbols. d.) When...

14) you are titrating 10.0mL of a solution of 0.25M acetic acid (Ka=1.8 x 10 ^-5)....

14) you are titrating 10.0mL of a solution of 0.25M acetic acid (Ka=1.8 x 10 ^-5). you are using a solution of 0.10M KOH to complete the titration curve. create the graph that would result by adding 1.0mL of the base to the acid and determining the pH and repeating until you have passed the equivalence point. Start the graph with 0 mL of the base solution added.

Sally chemist is attempting to determine the mass % of acetic acid in vinegar. Below is...

Sally chemist is attempting to determine the mass % of acetic acid in vinegar. Below is an excerpt from her lab book: A. Prepared vinegar analyte 25.0 mL vinegar mass of vinegar 25.20 grams added 75.0 mL H2O added 2 drops phenolphthalein temperature: 27.0 oC manufacturer's mass % acetic acid = 3.5 % B. Prepared burette filled with standardized NaOH solution 0.201 M C. Titration initial burette reading: 5.12 mL final burette reading: 78.67 mL solution is light pink 1....

As an Analytical chemist, you are designing a titration experiment to determine formic acid in food...

As an Analytical chemist, you are designing a titration experiment to determine formic acid in food samples (formic acid is used as a preservative and antibacterial agent). You test your protocol by performing a titration of 100.0 mL of 0.050 M formic acid (FW = 46.03 g/mol) with a 0.10 M sodium hydroxide standard solution. For formic acid Ka = 1.80 x 10−4 You can ignore activity coefficients! (60 points total) Vb = Volume of base added NOTE: Just providing...

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...

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