A solution was prepped by adding 0.7949 grams of silver (1) nitrate and 1.4721 grams of strontium (2) nitrate to a 250 ml flask and diluting it to the mark. Sodium sulfate (s) was added to the solution (no change in volume b/c negligible)
a. What percipitate will form first?
b. What is the conc. of the cation from the least soluble species when the second percipitate begins to fall out?
c. What is the max amount of pure compound (in grams) that can be recovered during this selective percipitation?
0.7949 grams of silver (1) nitrate is 170 g/mol = 0.0047 mole in 0.25L is 0.019 M
1.4721 grams of strontium (2) nitrate is 211.6 g/mol = 0.0069 mole in 0.25 L is 0.028 M
Ksp for strontium (2) sulfate is 3.44 x 10−7
Ksp for Ag(1) sulfate is 1.4×10–5
SrSO4 Sr2+(aq) + SO42-(aq)
Ksp = [Sr2+][SO42-]
3.44 x 10−7 = 0.028 x [SO42-]
[SO42-] = 3.44 x 10−7/ 0.028
[SO42-] = 1.23 x 10-5 M at this concentration of sulfate Sr2+ will pecipitate
Ag2SO4 2Ag+(aq) + SO42-(aq)
Ksp = [Ag+]2[SO42-]
1.4×10–5 =0.0192 x [SO42-]
[SO42-] = 0.0388 M at this concentration of sulfate Ag+ will pecipitate
a) Sr2+ will precipitate first
b) When Ag+ begins to precipitate Sr2+ will be
Ksp = [Sr2+][SO42-]
3.44 x 10−7 = [Sr2+] x 0.0388
[Sr2+] = 3.44 x 10−7 /0.0388
[Sr2+] = 8.87 x 10-6 M when silver begins to precipitate
So the amount of Sr that presipitates is 0.028 x 0.25 - 8.87 x 10-6 x 0.25 = 0.00689 moles of SrSO4 precipitates which is 0.00689 x 183.68 = 1.267 g
A solution was prepped by adding 0.7949 grams of silver (1) nitrate and 1.4721 grams of...
1) You need to make an aqueous solution of 0.125 M silver nitrate for an experiment in lab, using a 250 mL volumetric flask. How much solid silver nitrate should you add? ____ grams 2)How many milliliters of an aqueous solution of 0.160 M aluminum chloride is needed to obtain 6.50 grams of the salt? __ mL
What would the concentration of nitrate be (in M) in a solution prepared by adding 30.0 mL of 0.050 M potassium nitrate with 40.0 mL of a 0.075 M sodium nitrate solution into a volumetric flask that is 250 mL and then filling it up to the 250 mL mark with water and mixing it well?
1) In the laboratory a student combines 42.9 mL of a 0.482 M silver nitrate solution with 27.1 mL of a 0.592 M chromium(II) nitrate solution. What is the final concentration of nitrate anion ? 2)In the laboratory a student combines 40.1 mL of a 0.259 M magnesium nitrate solution with 23.3 mL of a 0.377 M magnesium chloride solution. What is the final concentration of magnesium cation?
Question 1 According to the following reaction, what mass of silver nitrate would be required to react with 0.500 grams of potassium chloride? AgNO3 (aq) + KCl (aq) --> AgCl (s) + KNO3 (aq) options 2.68 g 0.500 g 85.0 g 170 g 1.14 g Question 2 Consider the reaction: Na2CO3 (aq)+ 2 HCl (aq) --> 2 NaCl (aq) + CO2 (g) + H2O (l) If 43.41 g of sodium carbonate react completely, how many grams of HCl will be...
LAB VII. PRACTICE PROBLEMS - CHAPTER 4 NAME: SECTION: b) How many grams of strontium nitrate, Sr(NO), are needed to prepare 3.40x10 ml. of a 0.925 M solution? c) To what volume should 50.0mL of a 6.00M HCI stock solution be diluted to obtain a 1.50M HCl solution? How much water should be used? d) A 38.5ml sample of 0.875M AgNO, solution is mixed with 51.0mL sample of 0.744M NaCl solution. The AgCl precipitated has a mass of 2.06g. Calculate...
b. How would you prepare 225.0 mL of 1.33 M HCl from a 6.00 M stock solution? C. When 25.00 mL of 0.695 M HCl reacts with an excess of silver nitrate, will a precipitate form? Write the net ionic equation for this reaction. How many grams of precipitate can be theoretically obtained? d. What volume of 0.2500 M strontium hydroxide is required to completely react with 75.00 mL of 0.07942 M HCI? e. When 37.5 mL of 0.439 M...
4.30. Using solubility rules, predict the solubility in water of the following ionic compounds. a. AI(OH) b. CaN C. NH4CI d. KOH 4.32. Using solubility rules, decide whether the following ionic solids are soluble or insoluble in water. If they are soluble, write the chemical equation for dissolving in water and indicate what ions you would expect to be present in solution. (NE SO b. BaCO c. Pb(NOs)2 d. Ca(OH) 4.34. Write net ionic equations for the following molecular equations....
help please? this was the only other information given REPORT SHEET Determination of the Solubility-Product Constant for a Sparingly Soluble Salt EXPERIMENT 8 A. Preparation of a Calibration Curve Initial (Cro121 0.0024 M Absorbance 5 mL Volume of 0.0024 M K Cro Total volume 1. I mL 100 mL 2. 100ML 3. 10 mL 100ml 4. 15 mL 100 ML Molar extinction coefficient for [CrO2) [Cro,2) 2.4x100M 12x1044 2.4810M 3.6810M 0.04) 2037.37 0.85 1.13 2. 3. Average molar extinction coefficient...
please identify the unknown and write a derivative Unknown compound 3 Clear liquid Physcial Properties Solubility Dissolve in ethyl ether Not dissolved in water Boiling point 77 IR spectrum Transmitance 3000 1000 2000 Wavenumber cm-1) Classification Positive test in Alkaline Iron (III) Hydroxamate test test CLASSIFICATION TESTS These tests must be done together with known AND FOLLOW PROCEDURE IN YOUR TEXT CARBOXYLIC ACIDS are detected by teating aqueous solutions with limus or pH paper. Also, disolve In NaHCO with bubbles...