13.1-13.3) [References] Using the Bronsted-Lowry model, write an equation to show why the following species produce a basic aqueous solution. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank) HS (aq) + H20(1)

Solve for question 3a, b and c

In the laboratory, a general chemistry student measured the pH of a 0.386 M aqueous solution of ethylamine, C,H&NH, to be 12.094. Use the information she obtained to determine the K, for this base. K(experiment)- In the laboratory, a general chemistry student measured the pH of a 0.587 M aqueous solution of trimethylamine, (CH,),N to be 11.768. Use the information she obtained to determine the K, for this base. K,(experiment) =

In the following equations, identify the acids and bases in the forward and reverse reactions. Identify the conjugate acid-base pairs.   a NH3+H3PO4       <-> NH4+ + H2PO4- Acid   Base   Conjugate acid   Conjugate base   b H2PO4- + SO32- <-> HSO3- + HPO42- Acid   Base   Conjugate acid   Conjugate base   c CH3NH2 + CH3COOH            <-> CH3COO- + CH3NH3+ Acid   Base   Conjugate acid   Conjugate base

I Review | Constants | Periodic Table Learning Goal: Part A To calculate pH and use it as a measure of acidity. The pH expresses the molar concentration of hydronium ions in an aqueous solution on a logarithmic scale: What is the pH of an aqueous solution with [H30+] =2x10-14 M? Express the pH numerically using one decimal place. pH = -log[H3O+] • View Available Hint(s) [H3O+] = 10-pH As pH decreases, acidity increases. As pH increases, acidity decreases. • Acidic solution: pH 7 pH = Submit Part B Carbonated cola is more acidic than coffee or even orange juice because cola contains phosphoric acid. What is the molar concentration of H3O+ in a cola that has a pH of 3.120? Express your answer with the appropriate units. • View Available Hint(s) [H3O*] = Value Units Submit

[Review Topics] [References] Use the References to access important values if needed for this question Identify whether each species functions as a Brønsted-Lowry acid or a Brønsted-Lowry base in this net ionic equation. H,SO3 (aq) HS HSO, H,S (aq) Bronsted-Lowry Bronsted-Lowry Brønsted-Lowry Brønsted-Lowry In this reaction: The formula for the conjugate Mof H,SO3 is The formula for the conjugate of HS is Submit Answer Retry Entire Group 9 more group attempts remaining Cengage Learning Cengage Technical Support 98°F Rain coming

[Review Topics] [References] Use the References to access important values if needed for this questi In the following net ionic equation, identify each reactant as either a Bronsted-Lowry acid or a Bronsted-Lowry base. C18H2103N(aq) + H,O(1) → C13H21O3NH*(aq) + OH (aq) B-L B-L The formula of the reactant that acts as a proton donor is The formula of the reactant that acts as a proton acceptor is Submit Answer Retry Entire Group 8 more group attempts remaining Cengage Learning Cengage Technical Support 98 F Rain coming

In each row check off the boxes that apply to the highlighted reactant. The highlighted reactant acts as a... (check all that apply) reaction Brønsted-Lowry acid O Brønsted-Lowry base HCN(aq) + CH,NH,(aq) CN (aq) + CH,NH, (a9) O Lewis acid O Lewis base O Brønsted-Lowry acid O Brønsted-Lowry base HCH,CO2(aq) + NH (aq) → CH,CO,2 (aq) + NH (aq) A Lewis acid Lewis base Brønsted-Lowry acid Brønsted-Lowry base Ni(s) + 4 CO(g) → → Ni(CO)4(1) Lewis acid D' Lewis base Check Explanation O 2021 McGraw-Hill Educatic

2,4,7,8

I just need an answer. An explanation isn’t necessary, thank you.