Question

Bromophenol blue can be used as the indicator for the titration of hydrogen carbonate ion, a...

Bromophenol blue can be used as the indicator for the titration of hydrogen carbonate ion, a weak base, with HCl, a strong acid. This reaction can be represented by the following equation:

HCO3- (aq) + H+ (aq) --> H2CO3 (aq)

The equivalence point of this titration occurs at about pH 3.8. Qualitatively describe the series of color changes that occur as this titration proceeds.

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Blood contains a buffer of carbonic acid (H2CO3) and hydrogen carbonate ion (HCO3-) that keeps the...
Blood contains a buffer of carbonic acid (H2CO3) and hydrogen carbonate ion (HCO3-) that keeps the pH at a relatively stable 7.40. What is the ratio of [HCO3-] / [H2CO3] in blood? Ka1 = 4.30x10-7 for H2CO3.
I have a question about titration. When the indicator (usually a WA or WB) changes color,what...
I have a question about titration. When the indicator (usually a WA or WB) changes color,what is the state of the indicator itself? i.e. if titrant = Strong Acid, titrand = Strong base. If the indicator is a weak acid, at the equivalence point is the indicator itself neutral? Protonated? Deprotonated?
1.) You will work with 0.10 M acetic acid and 17 M acetic acid in this...
1.) You will work with 0.10 M acetic acid and 17 M acetic acid in this experiment. What is the relationship between concentration and ionization? Explain the reason for this relationship 2.) Explain hydrolysis, i.e, what types of molecules undergo hydrolysis (be specific) and show equations for reactions of acid, base, and salt hydrolysis not used as examples in the introduction to this experiment 3.) In Part C: Hydrolysis of Salts, you will calibrate the pH probe prior to testing...
1.)Write the net-ionic equation for the following titration at the equivalence point Strong acid (HA) and...
1.)Write the net-ionic equation for the following titration at the equivalence point Strong acid (HA) and Strong Base (MOH) Weak acid (HB) and Strong Base (MOH) Weak base (B) and Strong acid (HA) 1. a) draw the titration curves for each of the following; be sure to show where the equivalence point, and midpoint would occur! Adding 100 mL of 1.0M NaOH to 50.0 mL of 1.0M HCl Adding 100 mL of 1.0 M NaOH to 50 mL of 1.0M...
Indicator Low pH color Transition pH range High pH color Thymol blue (first transtion) Red 1.2...
Indicator Low pH color Transition pH range High pH color Thymol blue (first transtion) Red 1.2 - 2.8 Yellow Methyl red Red 4.4 - 6.2 Yellow Bromothymol blue Yellow 6.0 - 7.6 Blue Thymol blue (second transition) Yellow 8.0 - 9.6 Blue Phenolphthalien Colorless 8.3 - 10.0 Fuchsia 1. Select all of the following statements that are true about the universal indicator used in this experiment A.The universal indicator is a single chemical compound. B. At pH 1.2 the indicator...
Titration 1: weak acid (CH3COOH) w/ strong base (NaOH) Titration 2: strong acid (HCl) w/ strong...
Titration 1: weak acid (CH3COOH) w/ strong base (NaOH) Titration 2: strong acid (HCl) w/ strong base (NaOH) - Concerning the above two titrations, answering the following questions: 1.) Calculate the theoretical equivalence point in terms of NaOH added for each of the titrations. Assume the concentration of acid is 0.81 M and the concentration of base is 0.51 M. 2.) Which equation can be used to find the pH of a buffer? Calculate the pH of a buffer containing...
1. For the titration of 25.0 mL of 0.1 M HCl (aq) with 0.1 M NaOH...
1. For the titration of 25.0 mL of 0.1 M HCl (aq) with 0.1 M NaOH (aq), at what volume of NaOH (aq) should the equivalence point be reached and why? If an additional 3.0 mL of 0.1 M NaOH (aq) is then added, what is the expected pH of the final solution? 2. What is the initial pH expected for a 0.1 M solution of acetic acid? For the titration of 25.0 mL of 0.1 M acetic acid with...
What volume of 0.5 M NaOH is needed to perform the titration of 30 mL of...
What volume of 0.5 M NaOH is needed to perform the titration of 30 mL of 0.1 M H3PO4? Question options: a) V = 12 mL b) V = 6 mL c) V = 18 mL d) V = 30 mL he pH at the equivalence point when a 0.20 M weak base (Ka = 9.1 x 10-7) is titrated with a 0.20 M strong acid is: Question options: a) pH = 2.9 b) pH = 1.7 c) pH =...
1. How many dissociated H+ ions are there in (3.2x10^-1) L of an aqueous solution whose...
1. How many dissociated H+ ions are there in (3.2x10^-1) L of an aqueous solution whose pH is 11.55? * Note: your answer is assumed to be reduced to the highest power possible. 2. A volume of 10.0 0 mL of an unknown concentration of acetic acid solution is neutralized by 38.50 mL of 0.236M sodium hydroxide solution. Determine the conventratino of the unknown acetic acid solution. 3. A solution is 0.047 M in nitrous acid, HNO2, has a pH...
Sodium hydrogen carbonate NaHCO3 , also known as sodium bicarbonate or "baking soda", can be used...
Sodium hydrogen carbonate NaHCO3 , also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl, which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl (aq) + NaHCO3 (aq) → NaCl (aq) + H2O (l) + CO2 (g) The CO2 gas produced is...