1. Classify the following reactions according to the 3 types of chemical reactions:a. HCl(aq) + NaOH(aq)→NaCl(aq) + H2O(1)b. Ba(OH)2(aq) + ZnCl2(aq)→BaCl2(aq) + Zn(OH)2(s)c. 2AGNO3(aq) + Mg(s)→Mg(NO3)2(aq) + 2Ag(s)d. HNO3(aq) + NH;(aq)→NH,NO;(aq) + H2O(1)e. 2Cu(s) + O2(g)→2CUO(s)f. CaCl2(aq)+K2CO:(aq)→2KCI(aq)+CaCO3(s)2. Calculate the maximum volume of 6 M HNO; which would be required to react with 0.350 gof Cu metal as shown in the initial equation (step 2)?3.If you used 2-3 mL of 6.0 M HNO3 to dissolve the sample of Cu (0.350 g), what volume of 4.0M NAOH would be required to neutralize the excess HNO3?4.Solid zinc is used in the last reaction to reduce the copper in the copper (II) sulfate solution toelemental copper. Identify 2 other metals that could be used to perform the reduction. Explainyour answer. Write a balanced chemical equation for each identified metal.5.Based on your research, which of these metals you think would be theJustify your answer using MSDS and costs effects.enest" metal to use?

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Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter4: Stoichiometry

Section: Chapter Questions

Problem 4.56PAE

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You are given a 1.50-g mixture of sodium nitrate and sodium chloride. You dissolve this mixture into 100 mL of water and then add an excess of 0.500 M silver nitrate solution. You produce a white solid, which you then collect, dry, and measure. The white solid has a mass of 0.641 g. a. If you had an extremely magnified view of the solution (to the atomic-molecular level), list the species you would see (include charges, if any). b. Write the balanced net ionic equation for the reaction that produces the solid. Include phases and charges. c. Calculate the percent sodium chloride in the original unknown mixture.
Sulfuric acid is listed in a catalog with a concentration of 95-98%. A bottle of the acid in the stockroom states that 1.00 L has a mass of 1.84 kg. To determine the concentration of sulfuric acid in the stockroom bottle, a student dilutes 5.00 mL to 500. mL She then takes four 10.00-mL samples and titrates each with standardized sodium hydroxide (c = 0.1760 M). (a) What is the average concentration of the diluted sulfuric acid sample? (b) What is the mass percent of H2SO4 in the original bottle of the acid?
94. Baking soda (sodium hydrogen carbonate. NaHCO3) is often used to neutralize spills of acids on the benchtop in the laboratory. What mass of NaHCO3 would be needed to neutralize a spill consisting of 25.2 mL of 6.01 M hydrochloric acid solution?
Antacids neutralize the hydrochloric acid in your stomach. What is the correct neutralization reaction of stomach acid with Milk of Magnesia (Mg(OH)2)(Mg(OH)X2) ? Select one: HCl+Mg(OH)2⟶H2O+MgCl2HCl+Mg(OH)X2⟶HX2O+MgClX2 2HCl+Mg(OH)2⟶2H2+O2+MgCl22HCl+Mg(OH)X2⟶2HX2+OX2+MgClX2 HCl+Mg(OH)2⟶HMg+ClOHHCl+Mg(OH)X2⟶HMg+ClOH 2HCl+Mg(OH)2⟶2H2O+MgCl22HCl+Mg(OH)X2⟶2HX2O+MgClX2 HCl+Mg(OH)2⟶HMg+2Cl(OH)2
April wants to demonstrate the chemical reaction: CuSO4 + Fe à FeSO4 + Cu. She has 1 teaspoon of copper sulfate (CuSO4), one iron nail, a plastic cup, and 1212 cup of water. How can she proceed with the experiment to demonstrate that the mass of copper cannot be created nor lost? A Step 1. Using the plastic cup, dissolve the copper sulfate in water. Step 2. Submerge the iron nail in this solution. Step 3. Wait 15 minutes until the nail is covered with a thick layer of copper. Step 4. Weigh the cup with the nail inside. B Step 1. Weigh the copper sulfate, iron nail, plastic cup, and water. Step 2. Using the plastic cup, dissolve the copper sulfate in water. Step 3. Submerge the iron nail in the solution and wait 15 minutes. Step 4. Take out the nail from the cup and weigh the nail and cup. C Step 1. Weigh the copper sulfate, iron nail, plastic cup, and water. Step 2. Using the plastic cup, dissolve the copper sulfate in water. Step 3. Submerge the iron…
Sodium phosphate dissociates when it dissolves in water. Na3PO4 (aq) --> 3 Na+ (aq) + PO43- (aq) If the concentration of the Na3PO4 solution is 0.033 mol/L, what is the concentration of the sodium ions? a. 0.011 mol/L b. 0.033 mol/L c. 0.066 mol/L d. 0.099 mol/L
A common way to determine the catalyst: limiting reactant ratio in a catalytic reaction is to report the amount of catalyst used in mol%. For example, 5 mol% catalyst means that the reaction uses 5% as much catalyst as the limiting reactant. Showing all your work, calculate the mol% of Pd used in this reaction where R and R’ = H. aryl halide mw: 185.02 g/mol phenyl boronic acid: 121.93 g/mol Pd acetate: 224.5 g/mol
Sr(s)+2HC1(aq) = SrC1 2 (aq)+H2(g) (R3.1) the following reactions use oxidation numbers Oxidation states) to show which chemical species have been oxidised and which have been reduced C1 2(aq) + 21 -(aq) = 2C1-(aq) +1 2(aq) (R3.2) 2HNO3(aq) + 6H1(aq)=2NO3(aq)+6H1(aq)= 2NO(g) + 31 2(aq) + 4H2O(1) (R3.3)
A solution of Mg(NO3)2 is prepared in 425 mL of water by adding 32.0 g Mg(NO3)2. What us the concentration of nitrate ion (NO3-) in this solution? (a) 0.216 M (b) 0.432 M (c) 0.508 M (d) 1.02 M
An iron ore sample contains Fe2O3 plus other impurities. A 752-g sample of impure iron ore is heated with excess carbon, producing 453 g of pure iron by the following reaction:Fe2O3(s) + 3C(s) → 2Fe(s) + 3CO(g)What is the mass percent of Fe2O3 in the impure iron ore sample? Assume that Fe2O3 is the only source of iron and that the reaction is 100% efficient.
what type of reaction is fe+h2so4=fe2(so4)3+h2
20. 50 ml of a 0.874 M HNO3 solution is diluted to 0.250 l. What is the concentration of the diluted solution ? a) 0.525 Mc) 0.350 M b) 0.175 M d) 4.37 M

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