You are using gravimetric analysis to determine the
concentration of calcium (Ca2+) in tap water. The calcium is
precipitated as calcium oxalate monohydrate upon addition of
ammonium oxalate to the tap water according to the following
reaction:
Ca +2 (aq) + C2O4 -2 (aq) → CaC2O4 ∙H_2 O
(s) Ksp = 1.3 x 10 -8
The protocol calls for addition of 25 mL of 1.0 M ammonium oxalate
to 25 mL sample. In order to ascertain the accuracy of your method,
you fortify a second tap water sample (25.0 mL) with calcium (2.00
mL of 0.100 M Ca2+) and precipitate the calcium as with the
original sample. Once the precipitate is collected and dried you
determine the following masses of calcium oxalate
monohydrate:
Sample - 0.0326 g precipitate
Fortified sample – 0.0597 g precipitate
Calculate the % recovery of the added calcium
You are using gravimetric analysis to determine the concentration of calcium (Ca2+) in tap water. The...
"Hard" water contains mainly salts of Ca2+ and Mg2+, both of which form many insoluble salts. You have a water sample and need to determine whether it contains Ca2+ and/or Mg2+. When you add ammonia to the solution, followed by ammonium chloride and ammonium oxalate, a white precipitate of CaC2O4 should form if Ca2+ is present. What is the purpose of adding the ammonium chloride to the reactant mixture? a. The chloride ion helps to form the calcium chloride precipitate....
A 267.8-g sample of ground water is analyzed for calcium. The Ca2+ in the sample is first precipitated and filtered-off as NH4CaPO4·7H2O. This precipitate is dried and heated, releasing water and ammonia to yield anhydrous calcium pyrophosphate (Ca2P2O7). The mass of Ca2P2O7 obtained is 0.0437 g. Give the calcium content of the ground water in parts per million (to three significant figures).
04 (a) Calcium ions can be determined by precipitation of the oxalate according to the equation: Ca2+ (aq) + C2O42- (aq) = CaC204 (s) The solid may then be filtered off, washed and oxalic acid is regenerated by the addition of excess sulfuric acid. The amount of oxalic acid is then quantified by titration using potassium permanganate according to the equation: H2C204 + MnO4 + H+ = CO2 + Mn2+ + H20 (unbalanced) In an experiment to find the concentration...
You need to perform gravimetric analysis of a water sample in order to determine the amount of Ag present. List three aqueous solutions that would be suitable for mixing with the sample to perform the analysis b. a. Would adding KNO3(aq) allow you to perform the analysis? Assume you have performed the analysis and the silver solid that formed is moderately soluble. How might this affect your analysis results? C. You need to perform gravimetric analysis of a water sample...
PRE-LABORATORY QUESTIONS, WATER: DETERMINING THE CONCENTRATION OF CALCIUM IONS IN WATER SAMPLES EXPT. SA HARD Prior to coming to lab, carefully read the entire experimental procedure that follows and write an outline of the procedure in your lab notebook IN YOUR OWN WORDS (do not simply copy). Then, add three tables for your titrations of the blank, tap water, and CaCl samples. Complete these problems and hand in gt the bexinning of the laboratory period. Show all work. EDTA is...
How do you calculate questions 1 - 8 for the data analysis section? A. Precipitation of CaC,O, H,O from the Salt Mixture Unknown number Trial 1 Trial 2 1. Mass of beaker (g) 59.45 59.45 5.oS Mass of beaker and salt mixture (g) 2. 3. Mass of salt mixture (g) I, oo oS 4. Mass of filter paper (g 5. Mass of filter paper and product after air-dried or oven-dried (g) 0, 35 6. Mass of dried product (g) 7....
Purpose: To calculate the amount of AgNO3 present in an unknown solution of water through the process of gravimetric analysis with NaCl. Background: Have you ever had difficulty lathering soap or find that the scum in your shower constantly needs to be removed? These are signs of “hard water.” Soap does not lather well in hard water because metal ions, such as Ca2+, form precipitates, creating “soap scum.” A precipitate is an insoluble compound that forms when soluble ions in...
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....