Perform stoichiometric calculations for reactions in solution. a.) A 10ml of 6M HCl (Hydrochloric acid) solution needs to be diluted to 3M HCl solution. How much water is needed to dilute the solution? b.) What volume should you dilute 133ml of a 7.90M CuCl2 (Copper(II)Chloride) solution so that 51.5 ml of the diluted solution contains 4.49g CuCl2?

Perform stoichiometric calculations for reactions in solution. a.) A 10ml of 6M HCl (Hydrochloric acid) solution needs to be diluted to 3M HCl solution. How much water is needed to dilute the solution? b.) What volume should you dilute 133ml of a 7.90M CuCl2 (Copper(II)Chloride) solution so that 51.5 ml of the diluted solution contains 4.49g CuCl2?

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter7: Chemical Energy

Section: Chapter Questions

Problem 134IP: On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado....

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On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
Sample: Saline 0.900% (m/v), in sodium chloride (NaCl). Data: M.A. (g/mol): Na = 22.9898; K = 39.0983; Cr=51.9961; Ag = 107.8682; Cl = 35.453; N=14.0067; O = 15.9994. Material available in the laboratory's warehouse: Reagents: distilled water; standardized solution of silver nitrate (AgNO₃), at a concentration of 0.09980 mols/L; Potassium chromate solution (K₂CrO₄) 1%; ammoniacal ferric alum solution [Fe(NH₄)(SO₄)₂] and; nitrobenzene (or cooking oil, alternatively); 0.1000 mols/L potassium thiocyanate (KSCN) standard solution. Glassware: beakers of all sizes available on the market; 50, 100, 150, 200 and 250 ml Erlenmeyers; 10.00 and 25.00 mL volumetric pipettes; 15.00 mL burette; 30.00, 50.00 and 100.00 mL volumetric flasks Calculate the molarity of saline, in terms of the NaCl concentration (concentration in mols/L). (a) 0.900 mols/L (b) 5.84 mols/L (c) 0.154 mols/L (d) 0.0154 mols/L
When mixing sodium chlorate solution (volume 1.0L, density 1.1614 g/ml, mass fraction 22%) with hydrochloric acid( 2L, density 1.0980 g/ml, mass fraction 20%) an antiseptic substance was released. Write and balance the Mentioned reaction and name this anticipatic substance.
KHP (aq)+NaOH (aq)-->NaKHP (aq)+H2O(l) Trial Vi (mL) Vf (mL) 1 36.19 48.56 2 3 A student masses out 1.096 grams of KHP, which is dissolved in 25.00 mL of DI water. This KHP solution is titrated with NaOH, as shown in the equation above. Calculate the molarity of the NaOH solution.
A student carried out an experiment trying to prepare tetra-methyl-ammonium tri-iodide.The student weighed 1.13 g tetra-methyl-ammonium iodide into a beaker containing 25 mL ethanol, and then added 1.57 g of iodine. The mixture was heated gently, whilst stirring, on a hotplate until tetra-methyl-ammonium iodide, a white powder, was completely dissolved. After the mixture was allowed to cool down to room temperature, the mixture was further cooled on ice. After filtration on a Buechner funnel, washing with diethyl ether and leaving it under vacuum suction for a couple of minutes, the student recovered the product and weighed it. The mass of the obtained tetra-methyl-ammonium triiodide was 1.62 g.What is the yield of the reaction in percent [%]? For the calculation, assume that the product is completely dry and pure, so there are no impurities like side-products, unreacted educts, or solvent residues.
Phosphorus pentachloride reacts with water to form hydrochloric acid and phosphoric acid (below). A solution is created by reacting 4.5 g of PCl5 (MW=208.2 g/mole) with excess H2O. How many moles of NaOH are needed to titrate the resulting solution to completion. PCl5 + 4 H2O ----->5 HCl + H3PO4
Consider the reaction below: Pb(NO3)2(aq) + 2NH4I(aq) --> PbI2(s) + 2NH4NO3 25 g of 5.0% NH4I (MW 145 g/mol) solution is mixed with 45 g 3.0% solution of Pb(NO3)2 (MW 331 g/mol). Determine the excess reagent and how many moles of it remain in the solution after the reaction.
1. Use the following data table and steps a-d below to calculate the concentration of the zinc carbonate. The mass of the filter paper alone (no ZnCO3) was 1.3457 g. The Zn(NO3)2 solution (10.00 mL) was mixed with 15.00 mL of the 1.00 M Na2CO3. a. Calculate the mass of zinc carbonate formed. b. How many moles of zinc carbonate formed? c. Calculate the moles of zinc in the zinc nitrate solution used. d. Calculate the concentration of the zinc in the zinc nitrate solution.
In an impure sample of table salt that weighed 0.8421 g when dissolved in water and treated with excess AgN03 formed 2.044 g of AgCl. Listing the percentage of NaCl is in the impure sample. What is the list of three sources of error in this experiment?
Is there any way that I can get some assistance with parts E, F and G? What are also the types of reaction?
Please help me find weight percentage of the unknown solution, Thank you in advance Data attached below: Data of unknown NaCl solution (by weight) weight of weighing bottle and solution: 34.91g weight of weighing bottle: 23.91g weight of the solution: 11.00g Initial buret reading 33.28ml Final buret reading: 43.26ml The volume of the solution; 9.98 ml The density of solution: 1.10 Weight % of unknow solution: ?
Watch this video of a double displacement experiment: https://www.youtube.com/watch?v=mph8Hq_75vU Write the balanced chemical reactions, including state of the matter What is the precipitate that forms, and which color is it?