One Erlenmeyer contains 50 mL of 0.1 M Na2CO3 solution, the other Erlenmeyer contains 50 mL of 0.1 M NaHCO3 solution. Answer the following questions when both solutions are titrated with 0.1 M HCI (F=1) solution separately: a) How much mL will be consumed if the phenolphthalein indicator is used? b) How much mL will be consumed if the methyl orange indicator is used?

One Erlenmeyer contains 50 mL of 0.1 M Na2CO3 solution, the other Erlenmeyer contains 50 mL of 0.1 M NaHCO3 solution. Answer the following questions when both solutions are titrated with 0.1 M HCI (F=1) solution separately: a) How much mL will be consumed if the phenolphthalein indicator is used? b) How much mL will be consumed if the methyl orange indicator is used?

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter24: The Standardization Of A Basic Solution And The Determination Of The Molar Mass Of An Acid

Section: Chapter Questions

Problem 2ASA: In an acid-base titration, 21.16 mL of an NaOH solution are needed to neutralize 20.04 mL of a...

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Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at pH 7), and phenolphthalein (end point at pH 9)â€”which would you select for the following acid-base titrations? (a) perchloric acid with an aqueous solution of ammonia (b) nitrous acid with lithium hydroxide (c) hydrobromic acid with strontium hydroxide (d) sodium fluoride with nitric acid
A 0.3012g sample of an unknown monoprotic acid requires 24.13mL of 0.0944MNaOH for neutralization to a phenolphthalein end point. There are 0.32mL of 0.0997MHCl used for back titration. a. How many moles of OH are used? How many moles of H+ from HCl? _______moles OH ________moles H+ b. How many moles of H+ are there in the solid acid? Use Eq.5. ____________ moles H+ in solid c. What is the molar mass of the unknown acid? Use Eq.4. ____________ g/mol
Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
In an acid-base titration, 21.16 mL of an NaOH solution are needed to neutralize 20.04 mL of a 0.0997 M HCl solution. To find the molarity of the NaOH solution, we can use the following procedure: First note the value of MH in the HCl solution. ____________M Find MOH- in the NaOH solution. Use Eq.3. ____________M Obtain MNaOH from MOH. ____________M
One Erlenmeyer contains 50 mL of 0.1 M Na2CO3 solution, the other Erlenmeyer contains 50 mL of 0.1 M NaHCO3 solution. Answer the following questions when both solutions are titrated with 0.1 M HCl (F=1) solution separately: a) How much mL will be consumed if the phenolphthalein indicator is used? b) How much mL will be consumed if the methyl orange indicator is used? please explain than solve
5. One Erlenmeyer contains 50 mL of 0.1 M Na2CO3 solution, the other Erlenmeyer contains 50 mL of 0.1 M NaHCO3 solution. Answer the following questions when both solutions are titrated with 0.1 M HCl (F=1) solution separately: a) How much mL will be consumed if the phenolphthalein indicator is used? b) How much mL will be consumed if the methyl orange indicator is used?
A mixture containing Na2CO3 and NaHCO3 is dissolved in water and titrated with 0.1 N HCl using phenolphthalein indicator. The consumption is 20 ml. It is then titrated with methyl orange indicator. HCl consumption is 75 ml. Find the %NaHCO3 in the sample? (NaHCO3:84g/mol, Na2CO3:108g/mol)
Consider the following indicators: dinitrophenol (pKIn = 3.5), bromothymol blue (pKIn = 7), thymolphthalein (pKIn = 10). Match each titration below with its most-likely best indicator. (A specific indicator choice may be used more than once.) Group of answer choices titration of HF with NaOH [ Choose ] dinitrophenol bromothymol blue thymolphthalein titration of RbOH with HNO3 [ Choose ] dinitrophenol bromothymol blue thymolphthalein titration of HI with KOH [ Choose ] dinitrophenol bromothymol blue thymolphthalein titration of NH3 with HBr [ Choose ] dinitrophenol bromothymol blue thymolphthalein
100ml of asample of water required 10 ml of N/10 acid for titrating using phenolphthalein indicator. A100 ml sample of water was again taken and methyl orange was used as indicator, when15ml of N/10 acid was required for neutralization. Interpret the results of alkalinities in ppm.
An acid-base indicator is usually a weak acid with a characteristic color in the protonated and deprotonated forms. Because bromocresol green is an acid, it is convenient to represent its rather complex formula as HBCG. HBCG ionizes in water according to the following equation: HBCG + H2O ⇌ BCG- + H3O+ (yellow) (blue) a. Write the Ka expression for bromocresol green based on the equation above. b. When [BCG-] = [HBCG], then show that the expression simplifies to Ka = [H3O+]. If you know the pH of the solution, then the [H3O+] and Ka can be determined. c. What would be the color of the solution if there were equal concentrations of HBCG and BCG-?
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How do i determine the ml of KOH? (Picture posted) A student used 9.925 x 10-2 mol/L hydrobromic acid to standardize an aqueous solution of potassium hydroxide and obtained the following titration data using phenolphthalein as an indicator: Concentration of HBr used: 9.925 x 10-2 mol/L Volume of HBr used: 25.00 mL Indicator: phenolphthalein Endpoint colour change: colorless to pale pink