4 Predict if the following pairs of ions will undergo reaction or not, based on solubility at 25°C. If they will, write the precipitationreaction which occurs between them.ZNCI2 and NaOHA. ZnCl2(aq) + NaOH(aq) → NaCI(aq) + Zn(OH)2(s)O B. ZnCl2(aq) + 2 NaOH(aq) → 2 NaCl(aq) + Zn(OH)2(s)O C. ZnCl2(aq) + NaOH(aq) → NaZn(aq) + CIOH(s)O D.ZnCl2(aq) + 2 N2OH(aq) → 2 NaCl(aq) + 2 ZnOH(s)O E. 2 ZNC12(aq) + 2 NaOH(aq) → 2 NaCl(aq) + 2 ZNOH(s)F. ZnCl2(aq) + 2 NaOH(aq) → NaC(aq) + 2 ZNOH(s)O G. ZnCl2(aq) + 2 N2OH(aq) → NaCl(aq) + Zn(OH)2(s)O H. No reaction

ZnCl2 and NaOH are both soluble in water and dissociate into their respective ions as follows:…

Answered: Predict if the following pairs of ions…

Predict if the following pairs of ions will undergo reaction or not, based on solubility at 25°C. If they will, write the precipitation reaction which occurs between them. ZnCl2 and NaOH

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 98QRT: Does the pH of the solution increase, decrease, or stay the same when you (a) Add solid sodium...

See similar textbooks

Related questions

Q: Write the balanced NET IONIC equation for the reaction that occurs when nitric acid and potassium…

Q: What change will be caused by addition of a small amount of Ba(OH) 2 to a solution containing CN-…

A: The solution is- H+(aq)+CN-(aq)↔HCN(aq) here Hydrogen ions are reacting with cyanide ions to form…

Q: Calculate [H3PO4], [H2PO4], [HPO42-], [PO4³-], [H3O+], [OH-], and [Cl] in a mixture that is…

Q: The equilibrium concentration of manganese(II) ion in a saturated manganese(II) carbonate soltion is

A: Since the ksp of MnCO3 is not given, we will take the standard ksp, that is 1.8×10-11.

Q: The preparations of two aqueous solutions are described in the table below. For each solution, write…

Q: he solution of ash of Mg (ash is formed when Mg reacts with oxygen gas) when added to water is…

A: The solution formed is ---> Basic ---> option(b)

Q: le chatelier's principle

A: Le Chatelier's principle (also known as "The Equilibrium Law") states that when a system experiences…

Q: The preparations of two aqueous solutions are described in the table below. For each solution, write…

Q: Identify the compounds that are more soluble in an acidic solution than in a neutral solution. CaF,…

A: The compounds given are CaF2, NaNO3, LiClO4, CdS and CuI2.

Q: The maximum amount of iron(II) hydroxide that will dissolve in a 0.128 M iron(II) acetate solution…

A: The solution is given below -

Q: Determine the pH when 0.05mole of CO2 is dissolved into 1L of water. When 0.03 mole of sodium…

A: The carbon dioxide is a gas that dissolves n water upto a certain extent. There exists an…

Q: A 25.0 mL sample of lithium hydroxide is completely neutralized by adding 30.0 mL of 0.100 mol/L…

A: Given: Concentration of H3PO4 is 0.100 mol/L Volume of phosphoric acid is 30.0 mL or 0.03 L Volume…

Q: The preparations of two aqueous solutions are described in the table below. For each solution, write…

A: The solutions given are,

Q: Calculate molar concentrations of Cl-, Al3+, SO42-, Na+, and Fe2+ in 500 mL of water. Added to this…

A: Molarity (M) :- Number of moles of solute dissolved in one litre of solution is defined as as molar…

Q: The preparation of an aqueous solution is described in the table below. For this solution, write the…

A: Acids: HF Bases: KOH At equilibrium : Other: KF Acids: H3O+ Bases : OH-

Q: A solution is made by dissolving 48.9 g of Ba(NO2)2 in 500.0 mL of water. As NO2¯ is a base, write…

A: Answer:- This question is answered by using the simple concept of hydrolysis of salt of weak acid…

Q: the reaction of a strong acid with a strong base produces a salt and another product what is the…

A: We need to determine the products of reaction between strong acid and strong base.

Q: Explain why equilibrium calculations are not necessary to determine ionic concentrations in…

A: The “ratio of the concentration of products to the reactants” at equilibrium is the equilibrium…

Q: Which of the following graphs best represents the change in the pH and the reaction quotient Q when…

A: Here we to predict the the nature of graph of reaction quotient ( Q ) versus time and the pH change…

Q: The preparation of an aqueous solution is described in the table below. For this solution, write the…

A: Given that, 1.2 mol of KOH is added to 1.0 L of 1.2 M HCH3CO2 solution. A general neutralisation…

Q: A chemist prepares a 0.50 M solution of NaF which gives a measured pH of 8.58; and also prepares a…

A: In the above question the acidic and basic behaviour of the different salts is dependent on the…

Q: The preparations of two aqueous solutions are described in the table below. For each solution, write…

A: The solutions given are,

Q: precipitation of lead(II) iodide from aqueous solution:

A: In this question asked the ionic equation for the precipitation of lead iodide from aqueous solution

Q: Which of the following solids would be more soluble in an acidic solution than in neutral water?…

A: To get this answer we have to add H+ to the salt then anion will react and if this anion convert…

Q: Write the ionic equation for the dissolution and the solubility product for each of the following…

A: Dissolution refers to the process in which solute dissolves in a solvent to form a…

Q: Complete and balance the precipitation reaction. Include physical states. Refer to the solubilities…

A: To balance chemical equation only coefficients needs to be changed which occurs before reactants and…

Q: Identify the compounds that are more soluble in an acidic solution than in a neutral solution. HgI,…

A: Strong-base-weak-acid salts, such as MgF2 .(soluble in acidic solution) That is because when these…

Q: ven a solution of acetic acid, with equilibrium net ionic equation (so only showing the ions in the…

Q: The preparation of an aqueous solution is described in the table below. For this solution, write the…

Q: 58 Specify which of these salts will undergo hydrolysis: KF, NANO3, NH,NO,, MgSO,, KCN, C,H;COONA,…

A: Soln

Q: Explain what is acid-base titration.

A: Titration is a technique in which unknown concentration of analyte/titrand is find out by titrating…

Q: For each of the following slightly soluble salts, write thenet ionic equation, if any, for reaction…

A: a.

Q: The preparations of two aqueous solutions are described in the table below. For each solution, write…

A: When an acid react with base , it forms salt along with water and the reaction is called…

Q: Predict the products when mixing the solutions of 2 mole HCI and 1 mole Ca(OH)2.

Q: Write a balanced net ionic equation to explain the observed pH for each of the following solutions:…

A: NH4Cl (aq) + H2O (l) <---------------------> NH3 (aq) + H2O (l) + HCl(aq) Ionic equation is :…

Q: The preparations of two aqueous solutions are described in the table below. For each solution, write…

A: Here we have to predict the acid ,base and other species present at the equilibrium in the following…

Q: Hydrocholic acid (13.5 mL of 0.235 M) is added to 431.0 mL of 0.0790 M Ba(OH)2 solution. what is the…

A: The moles of HCl and the Ba(OH)2 moles are first calculated. The balanced chemical equation is as…

Q: One strategy for dealing with the acidification of lakes is to periodically add powdered limestone…

A: The chemical reaction of carbonates and its equation

Q: Write a reversible reaction for the buffer decomposition of NH4 + into ammonia (NH3 + ) and H+ ion

A: Buffer solution: The buffer solution is an aqueous solution consisting of a mixture of a weak acid…

Q: Which of the following salts will produce an acidic solution when added to pure water? a. CsNO3 b.…

A: To find out the salt among the given salt which will give the acidic solution on dissolving in…

Q: Which of the following salts is more solubility in an acidic solution than in a neutral solution?…

A: Caso3 and na2so4 is more soluble in acidic medium than water

Q: Explain two industrial applications of acidic buffer solutions.

A: Introduction : Buffer solutions : Solutions which resist the change in pH when small amount of acid…

Q: This question is concerned with acid/base. The ionic product of water may be taken as 10-14…

A: Answer:- This question is answered by using the simple concept of calculation of hydrogen ion…

Q: Predict whether each of the following pairs of substances could function as a buffer system in…

A: Given Buffer System (a) HNO3 and KNO3 (b) HCN and NaCN (c) KCl and KCN (d)…

Q: Write the balanced NET IONIC equation for the reaction that occurs when nitric acid and sodium…

A: The chemical equations should be balanced in accordance with the law of conservation of mass. This…

Q: A weak acid, HOCI, is in solution with dissolved sodium hypochlorite, NaOCl. If HCl is added which…

A: (1) Buffer of HOCl and NaOCl is a good example of acidic buffer solution. When any small amount of…

Q: Based on the ion-product constant, calculate the concentration of OH- ions if the concentration of…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

Predict if the following pairs of ions will undergo reaction or not, based on solubility at 25°C. If they will, write the precipitation
reaction which occurs between them.
ZNCI2 and NaOH
A. ZnCl2(aq) + NaOH(aq) → NaCI(aq) + Zn(OH)2(s)
O B. ZnCl2(aq) + 2 NaOH(aq) → 2 NaCl(aq) + Zn(OH)2(s)
O C. ZnCl2(aq) + NaOH(aq) → NaZn(aq) + CIOH(s)
O D.ZnCl2(aq) + 2 N2OH(aq) → 2 NaCl(aq) + 2 ZnOH(s)
O E. 2 ZNC12(aq) + 2 NaOH(aq) → 2 NaCl(aq) + 2 ZNOH(s)
F. ZnCl2(aq) + 2 NaOH(aq) → NaC(aq) + 2 ZNOH(s)
O G. ZnCl2(aq) + 2 N2OH(aq) → NaCl(aq) + Zn(OH)2(s)
O H. No reaction

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Phenol, C6H5OH, is a weak organic acid. Suppose 0.515 g of the compound is dissolved in enough water to make 125 mL of solution. The resulting solution is titrated with 0.123 M NaOH. C6H5OH(aq) + OH(aq) C6H5O(aq) + H2O() (a) What is the pH of the original solution of phenol? (b) What are the concentrations of all of the following ions at the equivalence point: Na+, H3O+, OH, and C6H5O? (c) What is the pH of the solution at the equivalence point?
Consider all acid-base indicators discussed in this chapter. Which of these indicators would be suitable for the titration of each of these? (a) NaOH with HClO4 (b) acetic acid with KOH (c) NH3 solution with HBr (d) KOH with HNO3 Explain your choices.
Three students titrate different samples of the same solution of HCI to obtain its molarity. Below are their data. Student A: 20.00mLHCl+20.00mLH2O 0.100 M NaOH used to titrate to the equivalence point Student B: 20.00mLHCl+40.00mLH2O 0.100 M NaOH used to titrate to the equivalence point Student C: 20.00mLHCl+20.00mLH2O 0.100 M Ba(OH)2 used to titrate to the equivalence point. All the students calculated the molarities correctly. Which (if any) of the following statements are true? (a) The molarity calculated by A is half that calculated by B. (b) The molarity calculated by A is equal to that calculated by C. (c) The molarity calculated by B is twice that calculated by C. (d) The molarity calculated by A is twice that calculated by B. (e) The molarity calculated by A is equal to that calculated by B.
8.When a small amount of 12 M HNO3(aq) is added to a buffer solution made by mixing CH3NH2(aq) and CH3NH3Cl(aq), the pH of the buffer solution changes from 10.64 to 10.62. Which of the following equations represents the reaction that accounts for the fact that the pH does not change significantly when the HNO3(aq) is added? a) CH3NH2(aq) + H+(aq) → CH3NH3+(aq) b)CH3NH3+(aq) + H+(aq) → CH3NH42+(aq) c) NO3- (aq) + H+(aq) → HNO3(aq) d) OH- (aq) + H+(aq) → H2O(l)
6.Which solution has the greatest concentration of hydroxide ions? 1.0 M HCl 1.0 M NaCl 1.0 M NaOH 0.1 M Ca(OH)2
Consider the reaction between 50.0 mL of 0.10 M NaOH and 75.0 mL of 0.20 M HCI at 25°. Which of the following statements is TRUE? HCl is the limiting reactant. After the reaction, the concentration of Na* is equal to the concentration of Cl'. After the reaction, the concentration of Cl' is still 0.200 M because Cl' is a spectator ion. After the reaction, the concentration of Na* is greater than the concentration of H30*. The final solution has a pH 1.10.
Starting with 0.1 mol L−1 HNO2(aq), which one of the following operations would cause the pH of the solution to increase? (Ka for HNO2 is 4.5 x 10−4). Select all that apply. You may select more than one, one, or none of the options. a) adding some NaNO2 b) adding some HCl c) adding some NaCl d) adding some HNO2
Here is ph of the molarity of butyl chloride (C,H,CI) in a reaction vessel during a certain chemical reaction. Use this graph to answer the questions in the table below. у 0.030- 0.0247 olo 0.020- Ar M 0.015- 0.010- 0.005- 500 1000 1500 2000 2500 3000 seconds created x10 Is C,H,Cl being created or destroyed by the chemical destroyed reaction? neither created nor destroyed If C,H,Cl is being created or destroyed, what is the rate at which it is being created or destroyed 1200 seconds after the reaction starts? Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility
The solubility constant of lead (II) hydroxide [Pb(OH)2] is 1.2 x 10-15. If 100.0 g of this compound is dissolved in water what is the concentration of [OH-] and [Pb2+]? If 0.100 M NaOH is added what is the concentration of [OH-] and [Pb2+]?
A sample of acetic acid is titrated with a standardized NAOH solution. Before the end-point of the titration, which of the following must be true? HC,H3O, (aq) + NAOH (aq) → NaC,H3O2 (aq) + H2O (1) Note: [X] = molar concenctration of X %3D O [H+] > [OH-] [-HO] > [+H] O %3D [-HO] = [+H] O
consider the titration of 50.0 mL of 0.10 M acetic acid with NaOH. drag and drop each amount of NaOH added (to the acetic acid) Into the appropriate resulting pH. In other words, determine the pH of the final solution after each volume of NaOH has been added. Will the resulting solutions be acidic, basic, or neutral? Consider the stration of 50.0 ml of 0.10 M acetic acid (HC₂H₂O₂. K, -18 x 10) with NaOH. Drag and drop each amount of NaOH added to the acetic acid) into the appropriate resulting pH. In other words determine the pH of the final solution after each volume of NaOH has been added. Will the resulting solution be acidic, basic, or neutra? Acidic Neutral Basic Drag and drop your selection from the following list to complete the answer 25.0 mL (total) of 0.10 M NaOH has been added (the halfway point) 50.0 mL. (total) of 0.10 M NaOH has been added (the equivalence point) 10.0 mL (total) of 0.10 M NaOH has been added 60.0 mL (total) of 0.10 M NaOll has been added No NaOH has been…
1. Write the complete chemical equation for the reaction of a solution of sodium hydroxide and hydrochloric acid. 2. How many mL of 0.1 M HCI are required to react completely with 5 mL of 0.1 M NaOH? 3. If equal molar amounts of NaOH and HCl are mixed, when the reaction is completed what will be the chemical species in the resulting solution? 4. What will be the pH of the mixture in question 3, acidic, neutral, or basic? Explain. 5. Write the complete chemical equation for the reaction of a 0.1 M solution of acetic acid (CH3COOH) with a 0.1 M solution of NaOH? 6. How many mL of the 0.1 M NaOH solution will be required to react completely with 5 ml of a 0.1 M acetic acid solution? Explain.