Classes of Chemical Reactions Pre-laboratory questions 1. Characterize each of the following as soluble or insoluble in water using the solubility rules: а) СаСОз b) NH,CIO4 c) Hg(NO;)2 d) K3PO4 2. For each of the following precipitation reactions, complete the reaction, balance the reaction, and determine the phases of the products using the solubility rules. a) Mg(NO3)2(aq) + NaOH(aq) → b) BaCl2(aq) + (NH4)2SO4(aq) → 3. Complete and balance the following acid-base reaction. Also label the Arrhenius acid and the Arrhenius base in the reaction. HCIO4 + Mg(OH)2 → 4. Balance the following redox reaction under acidic conditions. Cr2072-+ Fe2+ → Cr³+ + Fe³+

Classes of Chemical Reactions Pre-laboratory questions 1. Characterize each of the following as soluble or insoluble in water using the solubility rules: а) СаСОз b) NH,CIO4 c) Hg(NO;)2 d) K3PO4 2. For each of the following precipitation reactions, complete the reaction, balance the reaction, and determine the phases of the products using the solubility rules. a) Mg(NO3)2(aq) + NaOH(aq) → b) BaCl2(aq) + (NH4)2SO4(aq) → 3. Complete and balance the following acid-base reaction. Also label the Arrhenius acid and the Arrhenius base in the reaction. HCIO4 + Mg(OH)2 → 4. Balance the following redox reaction under acidic conditions. Cr2072-+ Fe2+ → Cr³+ + Fe³+

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The steps for determining the concentration of a sample of hydrochloric acid are listed below :Step (1): A 0.1038 M standard sodium carbonate solution was prepared by dissolving 2.750 g ofanhydrous sodium carbonate solid in deionised water and made up to 250.0 cm3.Step (2): 25.0 cm' of the standard solution obtained in Step (1) was transferred to a clean conical flask andthen a few drops of methyl orange were added.Step (3): The sample of hydrochloric acid was put into a burette. The standard solution in the conicalflask was titrated with the hydrochloric acid.Step (2) and Step (3) were repeated for several times. The table below shows the results of the titrations:Trial I 2 3 4Final burette reading/ cm330.85 28.75 28.30 31.35 27.25Initial burette reading/ cm32.00 1.50 1.00 3.00 0.00(a) Describe the procedure in preparing the standard sodium carbonate solution in Step (I). (b) State the colour change at the end point of the titration. (c) Calculate a reasonable average for the volume…
5. For each of the following equations, balance them, put in the missing solubility states and then write the net ionic equations. CdCl2( Ednanou Cd(s) + HCI(aq) - H2(g) + a. slueeloM ebrsled bns elolgmo nge acnom b. Fe(CIO3)2() + NaBr(L) → FeBr2( NaCIO3 (L)
Mark and John, two vinegar enthusiasts, are each tasked to determine the acetic acid content of their respective vinegar concoctions by titration. First, a 1 M-labeled KOH solution was standardized against the KHP (MW = 204.22 g/mol) standard that is 99.4% pure. In the process, 0.540 g KHP was found to require 2.80 mL of the KOH solution to completely react up to the phenolphthalein endpoint. Then, Mark and John both prepared their samples by taking 10.0-mL aliquots of each vinegar and diluting them to 25.0 mL. Using the same titrant and indicator, Mark’s vinegar required 18.60 mL of the standardized titrant to reach the endpoint, while John’s vinegar required 16.50 mL of the same titrant to reach the same endpoint. Question: What is the acetic acid concentration of Mark’s and John’s vinegar in molarity given that the Concentration of KOH is 9386 M?
Which of the following solutions could be used to separate the anions So42- and CO32- trom each other by precipitation? NANO3(ag) AGNO3(aq) Fe(NO3l3(aq) Ba(NO3)2(aq) Question Completion Status: A Click Submit to complete this assessment. Question 5 Fe(NOgl3 could be used to separate the anions PO4 and OH" from each other by precipitation. True False
to 70 ml of 0.2M Pb solution (NO3) 2 add 30 ml of 0.7 M KIO3 solution. a) Write the equation of the chemical reaction and calculate the number of moles of Pb2 + and IO3- ions before mixing b) count the number of moles of Pb2 + and IO3- ions after mixing, knowing that Ksp of Pb (IO3) 2 = 2.5 × 10-¹³
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What is the maximum mass (in grams) of each of the following soluble salts that can be added to 310 mL of 0.050 M BaCl2 without causing a precipitate to form? (Assume that the addition of solid causes no change in volume.) (a) (NH4)2SO4 ____ × 10___g (Enter your answer in scientific notation.) b) Pb(NO3)2 ______g c) NaF ______g
Table 1 - Solubility rules for ionic compounds in water Soluble Compounds 1. All alkali metal components (Group IA) are soluble. 2. All salts containing NH4+1, NO3-1, ClO4-1, ClO3-1 and C2H3O2-1 (acetate) are soluble. 3. All chlorides, bromides and iodides (Cl-1, Br-1 and I-1 respectively) are soluble except when combined with Ag+1, Pb2+ and Hg22+. 4. All sulfates (SO42-) are soluble except when combined with Pb2+, Ca2+, Sr2+, Hg22+ and Ba2+. Insoluble Compounds 5. All metal hydroxides and all metal oxides are insoluble except those in Group IA and those formed by Ca2+, Sr2+ and Ba2+. When metal oxides dissolve, they react with water to form hydrates. The oxide ion (O2-) does not exist in water. For example: Na2O(s) + H2O → 2 NaOH(aq) 6. All salts containing PO43-, CO32-, SO32-, and S2- are insoluble, except those in Group IA and NH4+1. Table 2 - Gases formed in metathesis reactions Gas Equation for formation H2S 2H+1 + S2- → H2S(g) CO2 2H+1 + CO32- → (H2CO3) →…
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Complete the table below by deciding whether a precipitate forms when aqueous solutions A and B are mixed. If a precipitate will form, enter its empirical formula in the last column. icrosoft O W W Microsoft Microsoft 6.52.210... esc solution A magnesium sulfate manganese(II) chloride potassium chloride Explanation ! < 8 2 solution B sodium hydroxide cadmium sulfate 9,214 barium bromide Check 280 3 Q Does a precipitate form when A and B are mixed? 103 O yes O yes NOV 1 yes 4 no no no % 5 empirical formula of precipitate ● 0 0 0 atv Google 6 3 09 & 7 X 2 00 © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility 9 Ś * 8 7 A nt ( 9 ) W 0 30 -DOCX + 11 - olo Ar 18 2 h E
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