Homework Answers
![To calculate fpH, we have to find out total [H] 1 H 1 the S04 - 4Son + 4 + full lonization is taking place 10.1 - 18.1 +10.1](http://img.homeworklib.com/questions/ccab5e80-d087-11eb-b740-b3bac2a7f9a9.png?x-oss-process=image/resize,w_560)
![So, total conch of H+ = [ht] from both equations = 18.1+ w = 18.4 + 0.46 = 18.56 Now, JH = -log [ht] - log (18-56) - - l. 269](http://img.homeworklib.com/questions/cdbf0fe0-d087-11eb-9fd7-c7a69491f562.png?x-oss-process=image/resize,w_560)
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instructions 1 pts Question 4 Concentrated sulfuric acid is 18.1 M. The first hydrogen is a...
9. Sulfuric acid (H2S04), a diprotic acid, is a strong acid in its first deprotonation (deprotonation-...
9. Sulfuric acid (H2S04), a diprotic acid, is a strong acid in its first deprotonation (deprotonation- loss of H'). The first deprotonation is considered complete (complete ionization). It is, however considered a weak acid for its second deprotonation with a Ka value of 1.2 X 102, For a 0.0456 M H2S04(aq) solution determine: (16 pts total) a. The chemical reaction equations for the successive loss of protons. (4 pts b. The concentration of HSO4-1 and H (H30') after the first...
Problem Set 15 CHEM 1252 November 10, 2019 4. A 0.100 M solution of bromoacetic acid...
Problem Set 15 CHEM 1252 November 10, 2019 4. A 0.100 M solution of bromoacetic acid (BrCH COH) is 13.2% Ionized dissociated). (a) Calculate [H3O+] (or "[*]"), [BrCH.CO." ] (or "[A-]"), and (BrCH2COH) (or "CHA]"). (b) Calculate K, and pk, for bromoacetic acid. 5. Ethylamine (CHCH NH) is a weak base in water. (a) Write a balanced chemical equilibrium reaction for the base hydrolysis of ethylamine. Label the acid, base, conjugate acid, and conjugate base. (b) Would you expect ethylammonium...
Question 6 4 pts Calculate the percent ionization of a 0.236 M solution of nitrous acid...
Question 6 4 pts Calculate the percent ionization of a 0.236 M solution of nitrous acid (a weak acid), with a pH of 1.53. Record to the hundredth's place.
1. Rank the solutions in order of decreasing [H3O+]: 0.10 M HF, 0.10 M HCl, 0.10...
1. Rank the solutions in order of decreasing [H3O+]: 0.10 M HF, 0.10 M HCl, 0.10 M HClO, 0.10 M HC6H5O. 2. The beaker will be filled to the 0.50 L mark with a neutral solution. Set the pH to 3.95 by using the green arrows adjacent to the pH value indicated on the probe in the solution. Once you adjust the pH, note the corresponding OH− ion concentration in M as given in the graphic on the left side...
(1 point) a) Calculate the pH of the following solutions of weak acids: i) 0.095 M...
(1 point) a) Calculate the pH of the following solutions of weak acids: i) 0.095 M propionic acid, K. = 1.3*10% ii) 0.0085 M phenol, K. = 1.3*100 b) Calculate the pH of 0.1 M sulfuric acid, being a strong acid for giving away the first H', and K, for the second step is 1.2*10? (2 points) c) Calculate the pH of a 0.1 M aqueous solution of NaCN. NaOH is a strong base, while the K. of HCN is...
< Homework 42 Weak Acid / Weak Base Equilibrium + Percent Ionization 2 of 8 Constants...
< Homework 42 Weak Acid / Weak Base Equilibrium + Percent Ionization 2 of 8 Constants Periodic Table Percent ionization can be used to quantify the extent of ionization of an acid in solution and is defined by the following formula for the acid HA: A certain weak acid, HA, has a Ka value of 4.7x10-7 Percent ionization=1 _HA ionized HA initial x 100% Part A Percent ionization increases with increasing K. Strong acids, for which K, is very large,...
Question 4 10 pts 4. Consider the titration curves (labeled a and b) for two weak...
Question 4 10 pts 4. Consider the titration curves (labeled a and b) for two weak acids, both titrated with 0.100 M NaOH: (0) Which acid solution is more concentrated? (ii) Which acid has the larger K? Hd pH TTTTTT TTTTTTT 0 20 40 60 80 100 Volume of base added (mL) 0 () 20 40 60 80 100 Volume of base added (mL) HTML Editore BIVA-A- IE111xx, 3. DO VIVO 12pt MacBook Pro
0.3931 0.34:1 12:1 D Question 5 5 pts A 25.0 mL sample of 0.150 M hydrofluoric...
0.3931 0.34:1 12:1 D Question 5 5 pts A 25.0 mL sample of 0.150 M hydrofluoric acid is titrated with a 0.150 M NaOH solution. What is the concentration of [F 1. Kb.[OH formed from the weak base ionization, and pH at the equivalence point? The K, of hydrofluoric acid is 3.5 x 10 In the space below enter your numerical answers in order of 1 to 4 include units. 1- Molarity of the Fluoride ion formed 2. The numerical...
It's a weak acid strong base titration Experiment 4: Identification of an unknown acid by titration...
It's a weak acid strong base titration
Experiment 4: Identification of an unknown acid by titration Page 2 of 15 Background In this experiment, you will use both qualitative and quantitative properties to determine an unknown acid's identity and concentration. To do this analysis, you will perform a titration of your unknown acid sample-specifically a potentiometric titration where you use a pH meter and record pH values during the titration, combined with a visual titration using a color indi- cator...
Question 4 2 pts If 11 drops of a formic acid (HCOOH) solution are titrated with 10 drops of a 0.12 M NaOH solution, what is the percent ionization of the formic acid solution? (Ka for formic aci...
Question 4 2 pts If 11 drops of a formic acid (HCOOH) solution are titrated with 10 drops of a 0.12 M NaOH solution, what is the percent ionization of the formic acid solution? (Ka for formic acid 1.78 x 104) 4.0% 1.3% 1.9% @ 2.5% Question 5 2 pts What is the pH of an acetic acid solution if 25 drops are titrated with 44 drops of a 0.45 M KOH solution? (K, for acetic acid 1.8 x 105)...
9. Sulfuric acid (H2S04), a diprotic acid, is a strong acid in its first deprotonation (deprotonation- loss of H'). The first deprotonation is considered complete (complete ionization). It is, however considered a weak acid for its second deprotonation with a Ka value of 1.2 X 102, For a 0.0456 M H2S04(aq) solution determine: (16 pts total) a. The chemical reaction equations for the successive loss of protons. (4 pts b. The concentration of HSO4-1 and H (H30') after the first...
Problem Set 15 CHEM 1252 November 10, 2019 4. A 0.100 M solution of bromoacetic acid (BrCH COH) is 13.2% Ionized dissociated). (a) Calculate [H3O+] (or "[*]"), [BrCH.CO." ] (or "[A-]"), and (BrCH2COH) (or "CHA]"). (b) Calculate K, and pk, for bromoacetic acid. 5. Ethylamine (CHCH NH) is a weak base in water. (a) Write a balanced chemical equilibrium reaction for the base hydrolysis of ethylamine. Label the acid, base, conjugate acid, and conjugate base. (b) Would you expect ethylammonium...
Question 6 4 pts Calculate the percent ionization of a 0.236 M solution of nitrous acid (a weak acid), with a pH of 1.53. Record to the hundredth's place.
(1 point) a) Calculate the pH of the following solutions of weak acids: i) 0.095 M propionic acid, K. = 1.3*10% ii) 0.0085 M phenol, K. = 1.3*100 b) Calculate the pH of 0.1 M sulfuric acid, being a strong acid for giving away the first H', and K, for the second step is 1.2*10? (2 points) c) Calculate the pH of a 0.1 M aqueous solution of NaCN. NaOH is a strong base, while the K. of HCN is...
< Homework 42 Weak Acid / Weak Base Equilibrium + Percent Ionization 2 of 8 Constants Periodic Table Percent ionization can be used to quantify the extent of ionization of an acid in solution and is defined by the following formula for the acid HA: A certain weak acid, HA, has a Ka value of 4.7x10-7 Percent ionization=1 _HA ionized HA initial x 100% Part A Percent ionization increases with increasing K. Strong acids, for which K, is very large,...
Question 4 10 pts 4. Consider the titration curves (labeled a and b) for two weak acids, both titrated with 0.100 M NaOH: (0) Which acid solution is more concentrated? (ii) Which acid has the larger K? Hd pH TTTTTT TTTTTTT 0 20 40 60 80 100 Volume of base added (mL) 0 () 20 40 60 80 100 Volume of base added (mL) HTML Editore BIVA-A- IE111xx, 3. DO VIVO 12pt MacBook Pro
0.3931 0.34:1 12:1 D Question 5 5 pts A 25.0 mL sample of 0.150 M hydrofluoric acid is titrated with a 0.150 M NaOH solution. What is the concentration of [F 1. Kb.[OH formed from the weak base ionization, and pH at the equivalence point? The K, of hydrofluoric acid is 3.5 x 10 In the space below enter your numerical answers in order of 1 to 4 include units. 1- Molarity of the Fluoride ion formed 2. The numerical...
It's a weak acid strong base titration
Experiment 4: Identification of an unknown acid by titration Page 2 of 15 Background In this experiment, you will use both qualitative and quantitative properties to determine an unknown acid's identity and concentration. To do this analysis, you will perform a titration of your unknown acid sample-specifically a potentiometric titration where you use a pH meter and record pH values during the titration, combined with a visual titration using a color indi- cator...
Question 4 2 pts If 11 drops of a formic acid (HCOOH) solution are titrated with 10 drops of a 0.12 M NaOH solution, what is the percent ionization of the formic acid solution? (Ka for formic acid 1.78 x 104) 4.0% 1.3% 1.9% @ 2.5% Question 5 2 pts What is the pH of an acetic acid solution if 25 drops are titrated with 44 drops of a 0.45 M KOH solution? (K, for acetic acid 1.8 x 105)...
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