Consider the reaction: HCl(ag) + NH3 (aq) = NH¸CI(aq) Where 20.00 mL of 0.100 M NH (aq) is added to 10.00 mL of 0.200 M HC1(aq). Order the solution components (excluding water) from highest to lowest concentration. [OH¯] > [NH3] > [Na*] > [Cl¯] > [H,O*] O [CI"] = [NH†] > [NH,] = [H,O*]> [OH"] O [H,O*)> [Cl¯]> [NH,] > [NH†] > [OH¯] O NH]= [OH¯] > [H,O*] = [Cl¯] > [NH3] O [H;O*] = [Cl¯]> [NH3] > [NH;] = [OH"] O [NH¸CI] = [NH,] = [HCl]

Consider the reaction: HCl(ag) + NH3 (aq) = NH¸CI(aq) Where 20.00 mL of 0.100 M NH (aq) is added to 10.00 mL of 0.200 M HC1(aq). Order the solution components (excluding water) from highest to lowest concentration. [OH¯] > [NH3] > [Na] > [Cl¯] > [H,O] O [CI"] = [NH†] > [NH,] = [H,O]> [OH"] O [H,O)> [Cl¯]> [NH,] > [NH†] > [OH¯] O NH]= [OH¯] > [H,O] = [Cl¯] > [NH3] O [H;O] = [Cl¯]> [NH3] > [NH;] = [OH"] O [NH¸CI] = [NH,] = [HCl]

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

You have a 350 mL solution that contains 0.015 M Ni2+ ions and 0.015 M Ca2+ ions. You slowly add Na2CO3 to the solution. What concentration of Na2CO3 must be added to precipitate the CaCO3 (Ksp = 5.0 × 10–9) from the solution without precipitating any NiCO3 (Ksp = 1.3 × 10–7)?
Benzoic acid, C6H5COOH, dissociates in water as shown in the equation below. A 40.0 mL sample of an aqueous solution of benzoic acid with a concentration of 0.50 M is titrated using standardized 0.25 M NaOH. C6H5COOH(s) -> C6H5COO–(aq) + H+(aq) Ka = 6.46 x 10^-5 Calculate the pH of the solution after the following amounts of NaOH have been added… A. 0 mL B. 10 mL C. 85 mL
An aqueous solution of 0.1 M H2SO4(aq) is added to 0.1 M Na2S(aq) and is allowed to react. From the following, select all of the statements that are true. The product of the reaction will have a colored supernatant The product of the reaction will have a colorless supernatant The reaction will produce water as a product The reaction will produce a precipitate The reaction will produce a gas The reaction will result in an oxidation and/or reduction of one of the reactants
A technician would like to standardize an unknown Ca(OH)2 solution. It takes 18.26 mL of a 0.191 M solution of HCl to titrate 25.00 mL the unknown Ca(OH)2 solution. Calculate the molarity of the Ca(OH)2 solution. Tip: Don't forget to consider the mole ratio between HCl and Ca(OH)2. 2HCl(aq)+Ca(OH)2(aq)⟶CaCl2(aq)+2H2O(l)
The end point in a titration of 50.00 mL of aqueous NaOH was reached by the addition of 35.23 mL of 0.250 M aqueous HCI titrant. Calculate the molarity of the NaOH solution. The titration reaction equation is: NaOH(aq) + HCI (aq) —> NaCl(aq) + H2O(l)
You have been provided with a 2.08 x 10-2 L sample of lithium hydroxide (LiOH) of unknown concentration. You perform a titration with 2.19 M nitric acid (HNO3), and find that 24.6 mL are required to reach the equivalence point (as determined using a coloured indicator). What is the concentration of the lithium hydroxide solution in mol L-1?
A student prepares a dilute solution of sodium hydroxide, NaOH (aq), starting with 6 M sodium hydroxide. She then titrates a 1.372 g sample of KHP with the dilute sodium hydroxide solution, NaOH (aq), to a phenolphthalein end point. A.) If the titration required 21.84 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of the sodium hydroxide solution, NaOH (aq). (Remember that KHP is potassium hydrogen phthalate, KHC8H4O4, NOT potassium hydrogen phosphorus!) B.) The student uses the same sodium hydroxide to titrate 10.00 mL of vinegar to a phenolphthalein end point. If the titration required 27.48 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of acetic acid, HC2H3O2 (aq), in the vinegar. C.) Calculate the mass percent of acetic acid, HC2H3O2 (aq), in the vinegar using the molar concentration for acetic acid, HC2H3O2 (aq), determined in part b and assuming the density of the solution is 1.01 g/mL.
Sodium hydroxide is extremely soluble in water. At a certain temperature, a saturated solution contains 565 g NaOH(s) per liter of solution. Calculate the molarity of this saturated NaOH(aq) solution.
Laura and Sebastian create an aqueous solution of Ba(OH)2 by pipetting 25.00 mL of 0.0970 M Ba(NO3)2 into an Erlenmeyer flask and that contains 25.00 mL of 0.105 M KOH. a) Calculate the molar concentrations of Ba2+(aq) and OH1-(aq) in their 50.00 mL solution. b) Use the molar concentrations of Ba2+(aq) and OH1-(aq) as determined above and the Ksp to show why a precipitate does not form. You must include a calculation as part of your answer. The value of Ksp for Ba(OH)2, is 5.0 x 10-3. c) Laura adds solid KOH to their solution of Ba(OH)2 until the hydroxide concentration, [OH1-], becomes 0.200 M. Assuming that the volume of the solution does not change, does the molar concentrations of Ba2+(aq) increase, decrease or remain the same? justify your answer.
Give detailed Solution...don't give Handwritten answer
Which of the following is TRUE about a 100.0 mL solution of 0.200 M Al2(SO4)3 (aq) ? There are 0.0600 moles of SO,2 (aq) ions in this solution. 4 This solution will contain three equivalents of Al2* (aq) ions and two equivalents of SO43 (aq) ions. There are 0.400 moles of Al3+ (aq) ions in this solution. The concentration of Al3+ (aq) ions in this solution is 0.200 M.
Consider a slightly soluble salt with a general form of MX2(s) --> M*(aq) + 2X(aq). If its molar mass is 121 g/mol and K, = 1.5 x 108, what is its solubility in grams per 100 mL? O 0.0015 g/100 mL O 0.019 g/100 mL O 0.15 g/100 mL O 0.55 g/100 mL,