Concept explainers
You are given a colorless unknown solution that contains one of the following salts:
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Chemical Principles in the Laboratory
- If 600 mL of some Pb(NO3)2 solution is mixed with 350 mL of 1.80 x 10−2 M NaCl solution, what is the maximum concentration of the Pb(NO3)2 solution added if no solid PbCl2 forms? (Assume Ksp = 2.00 x 10−5 M at this temperature.)arrow_forwardIron(III) sulfate is used as a coagulant for industrial waste. Write a dissociation equation andcalculate the concentration of the solute needed to produce a Fe2(SO4)3 (aq) solution with 0.600 mol/L iron(III) ionsarrow_forwardWhat mass of NaOHNaOH is needed to precipitate the Cd2+ ions from 30.0mL of 0.500 M Cd(NO3)2 solution?arrow_forward
- A 50.0 mL solution of Ca(OH) 2 with an unknown concentration was titrated with 0.340 M HNO3. To reach the endpoint, a total of 26.2 mL of HNO3 was required. Given that 0.00891 mol of HNO3 are used in the titration, What quantity in moles of Ca(OH)2 had to be present in the initial reaction?arrow_forwardEach row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. solution initial components A B с H₂O H₂O, NaOH H₂O, NaOH H₂O initial type (check all that apply) acidic basic neutral acidic basic neutral acidic basic neutral acidic basic neutral change add KI add NaBr add H Br add HI effect of change on pH (check one) pH higher pH lower pH the same pH higher pH lower pH the same pH higher pH lower pH the same pH higher pH lower pH the samearrow_forward1) An aqueous solution contains one or more of the following metal ions (and no others): Bi^3+, Cu^2+. Cr^3+, Mg^2+,Cs^2+. Outline a procedure to determine which ions are present and which ions are not present in the solution. 2) write a procedure to describe how a student can precipitate these ions: Ca^2+, Mg^2+arrow_forward
- A student is preparing 250 mL of a solution of 155.0 mM NaCl in 50.0 mM phosphate pH 6.4. The student has stock solutions of 0.850 M NaCl and 0.400 M phosphate pH 6.4. Calculate the volume of phosphate required to make the solution (in mL).arrow_forwardDetermine the concentrations of K₂SO4, K+, and SO42- in a solution prepared by dissolving 2.60 x 10-4 g K₂SO4 in 2.00 L of water. Express all three concentrations in molarity. Additionally, express the concentrations of the ionic species in parts per million (ppm). Note: Determine the formal concentration of SO42-. Ignore any reactions with water. [K₂SO₂] = [K+] = $ 4 [SO] = R F V % 5 T G B A 6 MacBook Pro Y H & 7 N U J M M * 00 8 [K+] = M [SO] = M ( 9 D I K H < V - O * ) O L command - P . V - I - : ; option { [ ? + 11 = 11 I ppm ppm } ] delete rearrow_forwardCalculate the molar concentration of Ag+ ion in a solution that has a pAg of 5.673. What is the molar concentration of K+ ion in a solution that contains 55.6 ppm of K3Fe(CN)6 (329.3 g/mol) Describe the preparation of 750 ml of 0.0650 M Cl- ion solution from solid BaCl2.2H2O (244.3 g/mol). Calculate the molar concentration of ethanol, C2H5OH, in an aqueous solution that contains 3.40 g of C2H5OH (46.07 g/mol) in 4.30 L of solution. How many moles of HCl are in 30.6 g HCl? Express your answer in millimoles. What is the mass in milligrams of the solute in 25.0 ml of 0.275 M NaOH?arrow_forward
- Fill in the missing words With the given plot, if a 0.1000 M NaOH solution was used to fully precipitate all the Zn2+ in the form of Zn(OH)2 with the addition of 6.00 mL of NaOH, the number of moles of Zn2+ in this 10 mL brass stock solution is mmol. Therefore, there are mmol of Zn2+ in the entire 100-mL brass stock solution, which is g/mol). mg of Zn2+ (FW = 65arrow_forwardCalcium oxalate, CaCO4, is very insoluble in water. What mass of sodium oxalate,Na2C2O4, is required to precipitate the calcium ion from 37.5 mL of 0.104 M CaCl2solution?arrow_forwardYou prepare a standard NaOH solution for the laboratory, using potassium hydrogen phthalate (KHC₈H₄O₄, abbreviated KHP) as the primary standard. KHP (molar mass = 204.22 g/mol) has one acidic hydrogen. It took 31.55 mL of the NaOH solution to titrate (react exactly with) 0.750 g KHP. You then use the standard base solution to determine the amount of ascorbic acid in a 500.0 mg tablet of vitamin C. Ascorbic acid (HC₆H₇O₆, molar mass 176.12 g/mol) also has one acidic hydrogen, and is usually mixed with some filler in preparing the tablets. It requires 17.54 mL of the NaOH to titrate (react exactly with) the ascorbic acid found in one 500.0 mg tablet. What is the percent vitamin C by mass in the tablet?arrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning