Homework Answers
For SrC2O4, it has a solubility of:
S = 5.66x10 ^ -4 mol / L
The Kps is calculated:
Kps = [Sr + 2] * [C2O4-2] = (5.66x10 ^ -4) ^ 2 = 3.20x10 ^ -7
The molarity of KMnO4 is calculated:
[KMnO4] = Ca * Va / Vb = 5.66x10-4 M * 50 mL / 7.50 mL = 3.77x10 ^ -3 M
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Fill in the blanks and Show all work Identity of SrC2O4 salt :_________ Solubility :__________ Ksp...
can u okease check if my calculations are correct and answer the bottom question with work...
can
u okease check if my calculations are correct and answer the bottom
question with work thank you
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Pre-Lab for Determination of Solubility Product Constant 1. Write the solubility product constant (Ksp) for the...
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Experiment 17A. A Solubility Product Constant Procedure Getting Started 1. Obtain a 10 ml pipet, ...
question#1
Experiment 17A. A Solubility Product Constant Procedure Getting Started 1. Obtain a 10 ml pipet, a 50 mL buret, and 2 pieces of 120 cm filter paper Preparing Saturated Solutions of M10J MIO), is an insoluble divalent iodate salt. The identity of the cation M-is unknown. 1 Prepare MIO,), by adding S0 ml of o.2 M KIO, to 20 mL of 1 Molar M(NO,J, in a 150 mt 2. Stir the mixture vigorously with a stirring rod. A white,...
help please? this was the only other information given REPORT SHEET Determination of the Solubility-Product Constant...
help please?
this was the only other information given
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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....
The titrant solution is on the last page. All the info needed is on the pages provided. paticularly on t...
The
titrant solution is on the last page.
All
the info needed is on the pages provided. paticularly on the last
page
Table 1: Standardization Data Trial 3 Trial 1 Trial 2 O.47644 0.4701 25. mL ou779 12.7mL 25. mL 12.4 mL Mass of KHP Initial burette reading 2.7mL 37,Sm 2.4m Final burette reading 12.7mL Volume of base used Data Analysis: 1. Write a balanced molecular equation (with phases, of course) for the reaction between the KHP and the titrant...
Fill in the data sheet and please show your work for the calculations Thermodynamics of Potassium...
Fill in the data sheet and please show your work for the
calculations
Thermodynamics of Potassium nitrate dissolving in water
KNO3(s) ↔
K+ (aq) +
NO3-(aq
Determine the thermodynamic variables, ΔG, ΔH, and ΔS, for the
dissolving of KNO3 in water. You will find these
variables by creating a Van’T Plot, which is a graph of
lnK(sp) vs 1/T.
A set amount of KNO3 is weighed and dissolved in 25mL
of water and heated until all the KNO3 is
dissolved....
can
u okease check if my calculations are correct and answer the bottom
question with work thank you
128 Solubility Product Constant Identity of Oxalate Salt: Barium Oxalate no 9: 0.00939/100ML N 0.093g/h 00043g x 10ome SOL ndarmas Kur from Solubility (Show your calculations below) 12 X1D of Bal 204 0.045G/L = 225.34 glad I Baço Bult Lag) (204 Lug) minutos com bone to critiche 0.093 g/L 0,043 g Belz0yX Imol BEC204 0.00041271 mall ->[6412043 225.24ylmol ksp= [Ba?"] [c204] ky...
R Prelab Assignment for Lab 10: Determining the Solubility Product Constant (Kp) of a Salt Jamm n rer014 Lab section: Date: Name: Show your work when there are calculations, write units, and use the correct significant figures. 1) a) If the solubility product constant (K) of salt with formula A2B3 is 42 x 10-24 what is the molar solubility of this salt? Ksp-LA A.ZX10 108 A. B.1) 2A(a)38() Ksp- LAB-421 Cancc) As Bs (S)2n3 (g)382(0g) 24 100 13X 3A 8-3710...
Pre-Lab: Solubility and the Common-Ion Effect Name: (You must show work for credit) 1. The solubility of silver carbonate (mm is its Ksp? 275.745), is 33.5 mg/L. What is its molar solubility, and what A student preforming the lab for the solubility of calcium iodate, titrated a 10.00 mL sample of saturated calcium iodate solution with a 0.011 M sodium thiosulfate solution, The titration required 21.62 mL to turn the solution clear. What was the concentration of the iodate in...
Pre-Lab for Determination of Solubility Product Constant 1. Write the solubility product constant (Ksp) for the following reaction as a function of the concentrations of the products: Ca(103) (s) Ca²+ (aq) + 210,- (aq) 2. Ca(IO3)2 will ionize in water to produce 10, ions. The 10, ions will react with KI. Write the reaction for this reaction. 3. We will be using starch as an indicator. Why? 4. In this experiment, we will first produce Izby mixing calcium iodate with...
question#1
Experiment 17A. A Solubility Product Constant Procedure Getting Started 1. Obtain a 10 ml pipet, a 50 mL buret, and 2 pieces of 120 cm filter paper Preparing Saturated Solutions of M10J MIO), is an insoluble divalent iodate salt. The identity of the cation M-is unknown. 1 Prepare MIO,), by adding S0 ml of o.2 M KIO, to 20 mL of 1 Molar M(NO,J, in a 150 mt 2. Stir the mixture vigorously with a stirring rod. A white,...
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...
PRE-LABORATORY QUESTIONS Fully answer these questions in your laboratory notebook before coming to lab. Show all work for numerical calculations. 1. Write out the chemical equation and equilibrium constant expression (Law of Mass Action) for the acetic acid / acetate ion buffer system. Derive the Henderson-Hasselbach equation for this system. 2. Calculate the pH of a buffer solution made by adding 1.3230 g of sodium acetate trihydrate (NaC,H,O, 3H,O) to 50.00 mL of 0.1652 M acetic acid. Assume there is...
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....
The
titrant solution is on the last page.
All
the info needed is on the pages provided. paticularly on the last
page
Table 1: Standardization Data Trial 3 Trial 1 Trial 2 O.47644 0.4701 25. mL ou779 12.7mL 25. mL 12.4 mL Mass of KHP Initial burette reading 2.7mL 37,Sm 2.4m Final burette reading 12.7mL Volume of base used Data Analysis: 1. Write a balanced molecular equation (with phases, of course) for the reaction between the KHP and the titrant...
Fill in the data sheet and please show your work for the
calculations
Thermodynamics of Potassium nitrate dissolving in water
KNO3(s) ↔
K+ (aq) +
NO3-(aq
Determine the thermodynamic variables, ΔG, ΔH, and ΔS, for the
dissolving of KNO3 in water. You will find these
variables by creating a Van’T Plot, which is a graph of
lnK(sp) vs 1/T.
A set amount of KNO3 is weighed and dissolved in 25mL
of water and heated until all the KNO3 is
dissolved....
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