Which of the mixtures represents a shift in the forward direction? Please select 2 correct answers from the following choices. Mixture 1 - Reference Mixture 3- Additional potassium thiocyanate Mixture 2 - Additional iron (III) nitrate Mixture 4 Addition of sodium sulfite

Which of the mixtures represents a shift in the forward direction? Please select 2 correct answers from the following choices. Mixture 1 - Reference Mixture 3- Additional potassium thiocyanate Mixture 2 - Additional iron (III) nitrate Mixture 4 Addition of sodium sulfite

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...

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O CHEMICAL REACTIONS Predicting precipitation Complete the table below by deciding whether a precipitate forms when aqueous solutions A and B are mixed. If a precipitate will form, enter its empirical formula in the last column. solution A sodium hydroxide cadmium acetate sodium sulfide solution B ammonium nitrate iron(II) bromide copper(II) nitrate Does a precipitate form when A and B are mixed? O yes O yes O no O no yes no empirical formula of precipitate 0 0 P X O 0/5 S
(Q52) Suppose that a solution that is 0.0334 M in sodium chloride and a solution that is 0.0334 M in strontium nitrate are mixed. What (if any) precipitates will form? O Strontium nitrate and strontium chloride O Strontium chloride O No precipitate will form O Strontium chloride and sodium nitrate O Sodium nitrate
- Part C Write a balanced ionic equation for this acid-base reaction: Ca(OH)2 (aq) + 2CH3CO₂H(aq) → Express your answer as a chemical equation. Identify all of the phases in your answer. ΑΣΦ A chemical reaction does not occur for this question. Submit Request Answer Part D ? Write net ionic equation for this acid-base reaction: Ca(OH)2 (aq) + 2CH3CO₂H(aq) → Express your answer as a chemical equation. Identify all of the phases in your answer.
Sample Mass of Original Mixture (g) Mass of Watch Glass (g) Mass of Filter Paper (g) Mass of Watch Glass, Filter Paper, and Precipitate (g) Avery 2.023 31.997 0.220 32.949 Zachariah 1.992 27.391 0.198 28.164 Sample Results from addition of ZnSO4 to supernatant (Beaker 1) Results from addition of Na3PO4 to supernatant (Beaker 2) Avery No change Precipitate forms Zachariah Precipitate forms No change 3 ZnSO4(aq) + 2 Na3PO4(aq) Zn3(PO4)2(s) + 3 Na2SO4 What was the mass, in grams, of the limiting reactant in the original mixture for Avery’s experiment?
A solution contains 1.19×102 M ammonium carbonate and 1.39x102 M sodium sulfide. Solid nickel(II) nitrate is added slowly to this mixture. What is the concentration of sulfide ion when carbonate ion begins to precipitate? [sulfide] =| M
A solution contains 5.54x10 3 M sodium hydroxide and 1.26x10² M sodium sulfide. Solid iron(III) nitrate is added slowly to this mixture. What is the concentration of sulfide ion when hydroxide ion begins to precipitate? [sulfide] = M Submit Answer Retry Entire Group 7 more group attempts remaining
Suppose a 0.031M aqueous solution of sulfuric acid (H₂SO4) is prepared. Calculate the equilibrium molarity of SO4. You'll find information on the properties of sulfuric acid in the ALEKS Data resource. Round your answer to 2 significant digits. IM S P X
5:15 1 ull 4G Discussion Assignment #6 O o o INFO DISCUSSION Discussion Assignment #6 Due:Wednesday, 14 Oct 2020, 3:00 PM In titration, one solution is added to another solution until a chemical reaction between the components in the solutions has run to completion. The solution being added is called the titrant, and we say that it solution. The completion of the reaction is usually shown by a change of color caused by a substance called an indicator. used titrate the other A typical titration proceeds in the following way. A specific volume of the solution to be titrated is poured into an Erlenmeyer flask. For example, 15.0 mL of a sulfuric acid solution of unknown concentration is added to a 250 mL Erlenmeyer flask. An indicator is then added to the flask, which changes color when the reaction is complete. The titrant in this example is potassium hydroxide, having a concentration of 0.121 M. The titrant is added to a buret. After slowly adding the titrant to the flask, the reaction…
The following refers to a titration lab: Would using a wet beaker to measure out the standardized sodium hydroxide solution cause your calculated hydrochloric acid concentration to be smaller than the actual concentration, larger than the actual concentration, or have no effect? Explain your reasoning Would using a wet Erlenmeyer flask to hold the hydrochloric acid analyte cause your calculated hydrochloric acid concentration to be smaller than the actual concentration, larger than the actual concentration, or have no effect? Explain your reasoning.
Given: If you weigh out exactly 0.150 g of an unknown substance to be dissolved in the 100.00 mL volumetric flask, and the concentration of Fe(II) in the 50 mL volumetric flask is calculated to be 1.27 x 10-4 M a. what is the mass (in grams) of iron that you would have in a 100.0 g sample of an unknown substance? HINT GIVEN: You are back calculating from the [Fe(II)] in 50.00 mL to [Fe(II)] in 100.00 mL and then determine the grams of Fe(II) in the mass of unknown sample weighed out to place in the 100 mL flask, to finally be able to calculate the mass of iron in 100.0g of sample. (answer a )
CyF3 is a slightly soluble salt that dissociates into Cy3+ and F- ions. CyF3 is a slightly soluble salt. In a saturated CyF3(aq) solution, the concentration of F–(aq) is _____ . Report your answer in M with three decimal places without units (example answer: 0.567) Ksp(CyF3) = 6.97 × 10–4.