I need help understanding how to do this homework question. I've been out sick so I don't even know how to even begin to attempt this question. Question 9Net lonic Eqns with Acids and BasesDissociate all strong acids and bases. Leave together all weak acids and bases. Cross out spectator ions.Strong Acids and Strong Bases ionize 100% in aqueous solution.- HCl is a strong acid. In solution we write it as H30*(aq) + Cl (aq).- HF is a weak acid. In solution we write it as HF(aq).- KOH is a strong base. In solution we write it as K"(aq) + OH (aq).- NH; is a weak base. In solution we write it as NH3(aq).Exception: Since Ca(OH)2 is only slightly soluble we write it as Ca(OH)2(s).Below is a list of the 6 strong acids and 6 strong bases you should know. All other acids and bases are considered weak.Strong AcidsHCI, HBr, HIHNO,HCIO4Strong Bases|LIOH, NaOH, КОНCa(OH)2 slightly solubleBa(OH)2Sr(OH)2H2SO4A. Write a net ionic equation for the reaction that occurs when aqueous solutions of bariumhydroxide and nitric acid are combined.Be sure to specify states such as (aq) or (s).Use H3O for the hydronium ion.If a box is not needed leave it blank.If no reaction occurs leave all boxes blank and click on "submit".B. Write a net ionic equation for the reaction that occurs when aqueous solutions of nitrousacid and potassium hydroxide are combined.Be sure to specify states such as (aq) or (s).If a box is not needed leave it blank.If no reaction occurs leave all boxes blank and click on "submit".C. Write a net ionic equation for the overall reaction that occurs when aqueous solutions of hydrosulfuricacid and sodium hydroxide are combined. Assume excess base.Be sure to specify states such as (aq) or (s).If a box is not needed leave it blank.If no reaction occurs leave all boxes blank and click on "submit".++

Answered: Image /qna-images/answer/f3840109-36fd-430f-9017-29dda01cbed5.jpg

Write a net ionic equation for the reaction that occurs when aqueous solutions of barium hydroxide and nitric acid are combined. Be sure to specify states such as (aq) or (s). Use H3O* for the hydronium ion. Ifa box is not needed leave it blank. If no reaction occurs leave all boxes blank and click on "submit".

Write a net ionic equation for the reaction that occurs when aqueous solutions of barium hydroxide and nitric acid are combined. Be sure to specify states such as (aq) or (s). Use H3O* for the hydronium ion. Ifa box is not needed leave it blank. If no reaction occurs leave all boxes blank and click on "submit".

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter15: Solutions Of Acids And Bases

Section: Chapter Questions

Problem 15.122QE: A Liquid HF undergoes an autoionization reaction: 2HFH2F++F (a) Is KF an acid or a base in this...

See similar textbooks

Similar questions

A Liquid HF undergoes an autoionization reaction: 2HFH2F++F (a) Is KF an acid or a base in this solvent? (b) Perchloric acid, HCIO4, is a strong acid in liquid HF. Write the chemical equation for the ionization reaction. (c) Ammonia is a strong base in this solvent. Write the chemical equation for the ionization reaction. (d) Write the net ionic equation for the neutralization of perchloric acid with ammonia in this solvent.
Classify each of the following as a strong or weak acid or base. a NH3 b HCNO c Mg(OH)2 d HClO3
Students are often surprised to learn that organic acids, such as acetic acid, contain OH groups. Actually, all oxyacids contain hydroxyl groups. Sulfuric acid, usually written as H2SO4, has the structural formula SO2(OH)2, where S is the central atom. Identify the acids whose structural formulas are shown below. Why do they behave as acids, while NaOH and KOH are bases? a. SO(OH)2 b. ClO2(OH) c. HPO(OH)2
Hydrogen, H2S, and sodium acetate, NaCH3CO2 are mixed in water. Using Table 16.2, write a balanced equation for the acid-base reaction that could in principle, occur. Does the equilibrium lie toward the products or the reactants?
(a) What is the pH of a 0.105 M HCl solution? (b) What is the hydronium ion concentration in a solution with a pH of 2.56? Is the solution acidic or basic? (c) A solution has a pH of 9.67. What is the hydronium ion concentration in the solution? Is the solution acidic or basic? (d) A 10.0-mL sample of 2.56 M HCl is diluted with water to 250. mL What is the pH of the dilute solution?
Two strategies are also followed when solving for the pH of a base in water. What is the strategy for calculating the pH of a strong base in water? List the strong bases mentioned in the text that should be committed to memory. Why is calculating the pH of Ca(OH)2 solutions a little more difficult than calculating the pH of NaOH solutions? Most bases are weak bases. The presence of what element most commonly results in basic properties for an organic compound? What is present on this element in compounds that allows it to accept a proton? Table 13-3 and Appendix 5 of the text list Kb values for some weak bases. What strategy is used to solve for the pH of a weak base in water? What assumptions are made when solving for the pH of weak base solutions? If the 5% rule fails, how do you calculate the pH of a weak base in water?
The nickel(II) ion exists as [Ni(H2O)4]2+ in aqueous solution. Why is this solution acidic? As part of your answer, include a balanced equation depicting what happens when [Ni(H2O)6]2+ interacts with water.
3.102 Classify the following compounds as acids or bases, weak or strong. (a) perchloric acid, (b) cesium hydroxide, (c) carbonic acid, H2CO3, (d) ethylamine, C2H5NH2
Classify the solutions represented in Exercises 9.28 and 9.30 as acidic, basic, or neutral.
A base is a substance that dissociates in water into one or more ______ ions and one or more ________. a.hydrogen . . . anions b.hydrogen . . . cations c.hydroxide . . . anions d.hydroxide . . . cations
Explain the difference between a monoprotic acid, a diprotic acid, and a triprotic acid. Give an example of each.