You are given four test tubes each containing a clear, colorless solution. You know the four solutions are supposed to be A-0.1 M NaNO,, B-01 M Ba(NO C-0.1M NaCl, and D- 0.5 M HCL, but the labels are missing. In each of the following scenarios, determine what additional aqueous solution (from the stockroom below) you could add to both test tubes that would allow you to correctly label what solution was in what test tube (HINT: in other words, look for a solution that when added to both test tubes will cause a reaction in one and not the other). In each case, describe the observations you would make and write a net ionic equation for any reactions that would occur to support your answer. Stockroom Solutions 0.1 MK₂CO₂ 0.1M K PO 0.1 M KNO₂ OSM KON 0.1M Na CO₂ 0.1M Na 50 0.1 M Na S 0.1M Nal 0.1 M Mg(NO₂) 01 M BaCl₂ 0.1 M CaCl₂ 0.1 M CuSO 0.1 M AgNO₂ 0.1 M Pb(NO OIMANO 0.1 MZnCl₂ a. Test Tube A contains 0.1 M NaNO, and Test Tube B contains 0.1 M Ba(NO b. Test Tube C contains 0.1 M NaCl and Test Tube D contains 0.5 M HCI c. Test Tube A contains 0.1 M NaNO, and Test Tube C contains 0.1 M NaCl

You are given four test tubes each containing a clear, colorless solution. You know the four solutions are supposed to be A-0.1 M NaNO,, B-01 M Ba(NO C-0.1M NaCl, and D- 0.5 M HCL, but the labels are missing. In each of the following scenarios, determine what additional aqueous solution (from the stockroom below) you could add to both test tubes that would allow you to correctly label what solution was in what test tube (HINT: in other words, look for a solution that when added to both test tubes will cause a reaction in one and not the other). In each case, describe the observations you would make and write a net ionic equation for any reactions that would occur to support your answer. Stockroom Solutions 0.1 MK₂CO₂ 0.1M K PO 0.1 M KNO₂ OSM KON 0.1M Na CO₂ 0.1M Na 50 0.1 M Na S 0.1M Nal 0.1 M Mg(NO₂) 01 M BaCl₂ 0.1 M CaCl₂ 0.1 M CuSO 0.1 M AgNO₂ 0.1 M Pb(NO OIMANO 0.1 MZnCl₂ a. Test Tube A contains 0.1 M NaNO, and Test Tube B contains 0.1 M Ba(NO b. Test Tube C contains 0.1 M NaCl and Test Tube D contains 0.5 M HCI c. Test Tube A contains 0.1 M NaNO, and Test Tube C contains 0.1 M NaCl

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

A student needs to dilute a 0.47 M Pb(NO3)2 solution to make 77.0 mL of 0.22 M Pb(NO3)2. Set up the calculation by placing the values with the correct units into the equation. Then, calculate the volume, in milliliters, of the 0.47 M Pb(NO3)2 solution that is needed.
The three drawings below represent aqueous ionic solutions. Solution A has a total volume of 25 mL, solution B has a total volume of 50. mL, and solution C has a total volume of 100. mL. If each sphere represents 0.011 mol of ions, calculate the total molarity of solute.
In a beaker there are 100 mL of a 1M sodium hydroxide solution. If we add an HCl solution and both substances are in stoichiometric amount, how many mL will we need to add taking into account that the solution prepared is of 36% in weight (density=1.1789 g/mL)?
250 mL of a 1.9 M Mg(OH)2 solution is added to a beaker. How many moles of Mg(OH)2 were added? How many grams of Mg(OH)2 were added?
A student weighs out a 11.4 g sample of AI(CH3COO)3, transfers it to a 250. mL volumetric flask, adds enough water to dissolve it and then adds water to the 250. mL tick mark. What is the molarity of aluminum acetate in the resulting solution? Molarity = M
we can precipitate out solid lead (II) iodide from an aqueous lead(II) nitrate solution by adding potassium iodide. if we have 500. mL of 0.632 M lead(II) nitrate solution how much 1.50 M potassium iodide must we add to exacltly precipitate all the lead (II) ions? 0.211 L 461 mL 0.632 L 0.421 L 0.316 L or 1.19 L
Exactly 6.21 g of MgCl, (molar mass - 95.2 g/mol) was dissolved in water. An analysis indicated that the molarity of the solution was 0.320 M. What was the volume (in mL) of the solution? Report your answer to three digits - for example 155 or 85.4 and do not include the unit ml. 28
A chemist needs 225 mL of 2.3 M HCl. What volume of 12 M HCl must be dissolved in water to form this solution? (Ignore significant figures for this problem.)
What volume in mL of an 11.6 M HCIO, (100.5 g/mol) solution is needed to make 500.0 mL of a 7.59 M HCIO4 solution? Do not put units in your answer. Report your answer as a whole number (no decimal places).
You wish to make a 0.242 M hydrobromic acid solution from a stock solution of 12.0 M hydrobromic acid. How much concentrated acid must you add to obtain a total volume of 150 mL of the dilute solution?
1) Get two medium test tubes. Into one, place about 2 mL of a solution of copper (II) sulfate. Into the other add about 2 mL of a solution of sodium phosphate. Note the appearence of the two solutions and then mix them together noting any changes that have taken place. -Changes that take place -Balanced chemical equation -Balanced ionic equation -balanced net ionic equation
You need to make 120.0 mL of a 0.40 MNAC1 solution. You have solid NaCl and your lab partner has a 1.5 MNaCl solution. Explain how you each make the 0.40 M Nacl solution. (a) What mass of the solid NaCl should you dissolve in pure water in order to prepare 120.0 mL of 0.40 M solution? Mass of NaCl= (b) What volume of 1.5 MNAC1 solution should your partner mix with pure water in order to prepare 120.0 mL of 0.40 M solution? Volume = mL