In the first trial of part A of the procedure, the ratio of moles H2O/moles CaSO4 is found to be 1.93. In the second trial the ratio was found to be 1.98. Calculate the relative average deviation of the two trials. Should the student run another trial? 200 4 0 6.09 els of es Plot of Mass of Precipitate
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Calculate the relative average deviation of the two trials. Should the student run another trial?
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- 3 Bal, (aq)+ 2 Nag POq Caq) 7 BalPO42 + l6 Nal laq • Consider the reaction of 30.0mL of 0.270M Balz with 20.0 mL of 0.3ISM Naz PO4. Lwhat quantity in meles of Balz are preset in the solution? are produced /What quantitg in moles of precipitate E ali Bal were consumed based on the balanced chomical equation? 6) What auantity in males of Na3 Pla aro present in soluction? d) What quantity in moles of precipitate are paduced if all the Naz PO, were cansumed based on the balanced chemi.cal equation? e) which reactant is limisting f What mass (in g) of precipitate is firemed when the limiting reactant is considered?The calcium (AW= 40.08 g/mol) from a sample of limestone weighing 607.4 mg was precipitated as calcium oxalate hydrate (CaC204.H20, FW 146.12 g/mol) and ignited to calcium carbonate (CaCO3, FW= 100.09 g/mol) weighing 246.7 mg. (c) If the precipitate had been ignited at a higher temperature giving calcium oxide (CaO, FW= 56.08 g/mol), what would be its weight?Standardization of a sodium hydroxide (NaOH) solution against potassium hydrogen phthalate (KHP) yielded the following results: Mass of KHP, g Volume of NaOH, mL 0.7987 38.29 0.8365 38.96 0.8104 38.51 0.8039 38.29 MM KHP: 204.22 MM NaOH: 40.00 a. Calculate the mean molar concentration of sodium hydroxide. (First, compute the concentration of NAOH in each titration then compute for its mean/average value.) b. Calculate the standard deviation. Please provide solutions for your answers. If you have used your calculator for calculating for mean and standard deviation, you can just provide the formula with the values indicated.
- 1. A solution is known to contain 38.04 ± 0.03 mM KCl, and you have taken an aliquot of this solution using a pipette calibrated to deliver 20.013 ±0.006 mL. Determine the number of moles of KCl that are delivered in the aliquot, including the absolute uncertainly in that value. 2. You deliver the aliquot taken in problem 1 into a volumetric flask with a volume of 250.00 mL ± 0.02 % and dilute the solution to volume in the flask using Dl water. What is the concentration of KCl in this flask, report your answer with the absolute uncertainty. 3. Tabulated below are replicate titration volumes for an analysis. What is the error (both absolute and percent) for the average titration volume?b) A carbonate of metal X has the formular X,CO3. The carbonate reacts with hydrochloric acid according to the following equation: X,CO3 + 2HC! → 0.25g of X,CO3 was found to neutralize exactly 23.6cm³ of hydrochloric acid of concentration 0.15moldm? ( RAM for C=12;0=16) i) Calculate the number of moles of hydrochloric acid 2XCl + CO2 +H,0 ii) Calculate the number of moles of X,CO3 iii) Calculate the relative molecular mass of X,CO3 iv) Calculate the relative atomic mass of X and hence deduce its identity c) Propanoic acid is a weak acid with an acid dissociation constant of 1.22x 10°moldm i) Write an equation for the ionization of propanoic acid -3 ii) Calculate the pKa for propanoic acid Lo iii) Sodium propanoate is made by the titration using 0.1M sodium hydroxide with propanoic acid A: Write an equation for the reaction B: Name a suitable indicator for this titration iv) A mixture of sodium propanoate and propanoic acid acts as a buffer solution. What is a buffer solution?4. Predict the effect of temperature decrease, (b) pressure increase, (c) concentration increase of O2 on the concentration of all species. Answer using "more" or "less". 2 SO3(9) O2(9) + 2 SO2(9) AH = - 47 Kcal a. b. С.
- A 1.407 g sample of canned tuna was analyzed by the Kjeldahl method. The liberated NH3 required 26.45 mL of 0.1180 M HCl. Calculate the percentage nitrogen and protein in the sample. Assume that the protein factor is 6.25, i.e. % protein = % N x 6.25.can be used as a standard solution for checking the concentration of a solution containing sulphuric acid, 8.7 cm' of sulphuric acid. Find the concentration of the sulphuric acid in both mol dm3 and g dm³. In a particular experiment 10,0 cm³ of a 0.50 mol dm³ solution of sodium ethanedioate was found to react with Q2. Sodium ethanedioate, Na;C¿O4, can be made into a solution of an exact and reliable concentration and so London ndon A.C.1.2The aluminum in a 1.200-g sample of impure ammonium aluminum sulfate was precipitated with aqueous ammonia as the hydrous Al2O3.xH2O. The precipitate was filtered and ignited at to give anhydrous Al2O3, which weighed 0.2001 g. Express the result of this analysis in terms of %NH4Al(So4)2 %Al2O3 %Al
- Chemistry Tutorial O 2. (Based on Lime- soda process of water softening) QI. Calculate the amount of lime and soda required to soften 25,000 litres of water having following analysis: Ca(HCO, )2 4.86 ppm;Mg(HCO3)2 = 7.3 ppm;CaSO, 6.8 MgCl2 = 5.7 ppm; MgSO. = 9.0 ppm; SiO, = 3.5 ppm; NaCl = 5.85 ppm. (Ans. L = 490 g:S =490g) %3DVIII. A primary standard of HCI is sodium carbonate, Na2CO3. A measured mass of solid Na2CO3, mNa2CO3' in grams, is dissolved in water and then titrated with HCI solution using methyl 2 NaCl + CO2 + H2O. orange indicator. The reaction is: Na2CO3 + 2 HCI- Complete the following formulas using the context described above: MHCI × VHCI in mL at the methyl orange endpoint = mNa2CO3 × ( )= mol of Na2CO3 mol of Na2CO3 X (— ( - - )= mol of HClExcess (NH4)2SO4 ( NH 4 ) 2 SO 4 was added to a 70.0 mL 70.0 mL solution containing BaCl2 BaCl 2 (MW=208.23 g/mol). ( MW = 208.23 g/mol ) . The resulting BaSO4 BaSO 4 (MW=233.43 g/mol) ( MW = 233.43 g/mol ) precipitate had a mass of 0.2192 g 0.2192 g after it was filtered and dried. What is the molarity of BaCl2 BaCl 2 in the solution?