The ion HCO3- is amphoteric (can act as both a base and an acid when placed into water). Write th...
The ion HCO3- is amphoteric (can act as both a base and an acid when placed into water). Write the reaction that occurs in both instances. Include the correct charges on all ionic species.
HCO3- acting as an acid
HCO3- acting as a base
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The ion HCO3- is amphoteric (can act as both a base and an acid when placed into water). Write th...
Both HC_2O_e and HS are amphoteric. Write an equation to show how HC_2O_4 can act as...
Both HC_2O_e and HS are amphoteric. Write an equation to show how HC_2O_4 can act as a base with HS acting as can acid. Express your answer as a chemical equation. Identify all of the phases in your answer. Write equation to show how HC_2O_4 can act as an acid with HS acting as a base. Express your answer as a chemical equation, identify all of the phases in your answer.
24. The dihydrogen phosphate ion HSO3 can act as an acid or a base in water...
24. The dihydrogen phosphate ion HSO3 can act as an acid or a base in water solution. Label each species physical state [(s), (liq), (g), (aq)]. Show all work for full credit. (a) Write the reaction where HSO3" acts as an acid (K): (2 pts) (b) Write the reaction where HSO3" acts as a base (Kb): (2 pts)
A species that has the potential to act both as an acid and as a base...
A species that has the potential to act both as an acid and as a base according to Brønsted-Lowry Theory is said to be amphoteric. Consider the one of the following ions based on the FIRST letter of your LAST name and answer questions a-c: a. Is the ion amphoteric? b. What is its conjugate base if any? c. What is its conjugate acid if any? 1.
Arsenic trichloride can act both as a Lewis acid and as a Lewis base. Explain why...
Arsenic trichloride can act both as a Lewis acid and as a Lewis base. Explain why this is so and write a balanced equation for each using BF3 and Cl− as reaction partners. 1,Write the balanced equation with AsCl3 acting as Lewis base. 2,Write the balanced equation with AsCl3 acting as Lewis acid.
Like water, the hydrogen carbonate ion (HCO31-) is amphiprotic. That is, it can act like a...
Like water, the hydrogen carbonate ion (HCO31-) is amphiprotic. That is, it can act like a Bronsted-Lowry acid or as a Bronsted-Lowry base. Write equations to show both of these reactions with water
Writing polyprotic acid and base reactions: 1. Write all the dissociations for the three polyprotic acids:...
Writing polyprotic acid and base reactions: 1. Write all the dissociations for the three polyprotic acids: H_2CO_3, H_3AsO_4, H_3PO_4. Match the appropriate Ka1, Ka2, Ka3 values to the dissociation reaction. 2. Identify all the species in each of the reactions as either an acid, a base, or amphoteric. Imagine putting NaH_2AsO_4 in solution. This is a salt. Describe, using chemical equation, exactly what happens? First write the dissociation reaction of the salt. Then identify the pH active species, and then...
17. The hydrogen sulfate or bisulfate ion HSO4 can act as either an acid or a...
17. The hydrogen sulfate or bisulfate ion HSO4 can act as either an acid or a base in water solution (a) Show the reaction where HSO4 acts an acid (K). (b) Show the reaction where HSO4 acts a base (Kb)?
The strong acid H2SeO4 will completely ionize in water, however the conjugate base can then act...
The strong acid H2SeO4 will completely ionize in water, however the conjugate base can then act as a acid an ionize further. The second Ka, Ka2 for HSeO4 is 1.2 x 10-2. This second Ka is not insignificant, being stronger than many other weak acids. A. Calculate the [H3O+] for a solution of 0.150 M H2SeO4. B. Using the value calculated above, calculate the value of [H3O+] for both ionizations of the acid. Grading will be based on the...
1. Write a balanced equation for the reaction of HCN in water. Identify the acid, base, conjugate acid and conjugate base.
1. Write a balanced equation for the reaction of HCN in water. Identify the acid, base, conjugate acid and conjugate base.2. Write a balanced equation for the reaction of NH3 in water. Identify the acid, base, conjugate acid and conjugate base. 3. Write a balanced equation for the reaction of HPO42- in water (where HPO42- is acting as the acid). Identify the acid, base, conjugate acid and conjugate base.4. Write a balanced equation for the reaction of HPO42- 2 in...
Part A Write an equation to show how HC204 can act as a base with HS...
Part A Write an equation to show how HC204 can act as a base with HS acting as an acid. Express your answer as a chemical equation. Identify all of the phases in your answer. = ALO O ? Submit Request Answer Part B Write an equation to show how HC,04 can act as an acid with HS acting as a base Express your answer as a chemical equation. Identify all of the phases in your answer, AED - O...
Both HC_2O_e and HS are amphoteric. Write an equation to show how HC_2O_4 can act as a base with HS acting as can acid. Express your answer as a chemical equation. Identify all of the phases in your answer. Write equation to show how HC_2O_4 can act as an acid with HS acting as a base. Express your answer as a chemical equation, identify all of the phases in your answer.
24. The dihydrogen phosphate ion HSO3 can act as an acid or a base in water solution. Label each species physical state [(s), (liq), (g), (aq)]. Show all work for full credit. (a) Write the reaction where HSO3" acts as an acid (K): (2 pts) (b) Write the reaction where HSO3" acts as a base (Kb): (2 pts)
A species that has the potential to act both as an acid and as a base according to Brønsted-Lowry Theory is said to be amphoteric. Consider the one of the following ions based on the FIRST letter of your LAST name and answer questions a-c: a. Is the ion amphoteric? b. What is its conjugate base if any? c. What is its conjugate acid if any? 1.
Writing polyprotic acid and base reactions: 1. Write all the dissociations for the three polyprotic acids: H_2CO_3, H_3AsO_4, H_3PO_4. Match the appropriate Ka1, Ka2, Ka3 values to the dissociation reaction. 2. Identify all the species in each of the reactions as either an acid, a base, or amphoteric. Imagine putting NaH_2AsO_4 in solution. This is a salt. Describe, using chemical equation, exactly what happens? First write the dissociation reaction of the salt. Then identify the pH active species, and then...
17. The hydrogen sulfate or bisulfate ion HSO4 can act as either an acid or a base in water solution (a) Show the reaction where HSO4 acts an acid (K). (b) Show the reaction where HSO4 acts a base (Kb)?
Part A Write an equation to show how HC204 can act as a base with HS acting as an acid. Express your answer as a chemical equation. Identify all of the phases in your answer. = ALO O ? Submit Request Answer Part B Write an equation to show how HC,04 can act as an acid with HS acting as a base Express your answer as a chemical equation. Identify all of the phases in your answer, AED - O...
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