Classify the two reactions, write their net ionic equations, and identify the spectator ion(s) and species transferred during the reactions. (Note: In aqueous solution, H^(+) is more appropriately represented as H.(3)0^(+). However, for the sake of brevity, it is shown here as H^(+) .) (a) Mn(s) + 2HBr(aq)-> MnBr_2(aq) + H_2(g)Classify this reaction. ( Select all that apply.) acid-base reaction combustion reaction decomposition reaction direct combination double displacement reaction exchange reaction isomerization reaction oxidation-reduction reaction precipitation reaction single displacement reaction substitution reaction synthesis reaction Write the net ionic equation. (Include states-of- matter under the given conditions in your answer. Use the lowest possible whole number coefficients.) Identify the spectator ion(s). (Include states-of-matter under the given conditions in your answer. Separate substances in a list with a comma.) [[chemPad, (9) Help], [x (D),x^(D)-> larr

Classify the two reactions, write their net ionic equations, and identify the spectator ion(s) and species transferred during the reactions. (Note: In aqueous solution, H^(+) is more appropriately represented as H.(3)0^(+). However, for the sake of brevity, it is shown here as H^(+) .) (a) Mn(s) + 2HBr(aq)-> MnBr_2(aq) + H_2(g)Classify this reaction. ( Select all that apply.) acid-base reaction combustion reaction decomposition reaction direct combination double displacement reaction exchange reaction isomerization reaction oxidation-reduction reaction precipitation reaction single displacement reaction substitution reaction synthesis reaction Write the net ionic equation. (Include states-of- matter under the given conditions in your answer. Use the lowest possible whole number coefficients.) Identify the spectator ion(s). (Include states-of-matter under the given conditions in your answer. Separate substances in a list with a comma.) [[chemPad, (9) Help], [x (D),x^(D)-> larr

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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Plz explain the following:
The quantity of Cl^- in a municipal water supply is determined by titrating the sample with Ag^+. The precipitation reaction taking place during the titration is Ag^+ (aq) + Cl^- (aq) > AgCl (s). a) How many grams of chloride ion are in a sample of the water if 20.2 mL 0f 0.100M Ag^+ is needed to react with all tghe chloride in the sample? b) if the sample has a mass of 10.0g, what percentage of Cl^- does it contain?
Write the shorthand notation for the following reaction. Mn (aq) + 4 H2O (1) + 5 Ag* (aq) → 5 Ag (6) + MnO4 (aq) + 8 H* (aq)
Jack determines the concentration of NaOH by titrating it with 4.0 g KHP (a monoprotic acid). It takes 21.2 mL of NaOH to reach the equivalence point. What is the concentration of the NaOH? molar mass of KHP 204.2 g/mol [NaOH] = [?] M [NaOH], M Enter
Solution X containing 0.020 mol of iron(II) sulfate requires 22.5 mL of potassium manganate(VII) for a complete reaction. The equation for the reaction is: 5Fe^2+ + MnO4^- + 8H^+ → Mn^2+ + 4H2O + 5Fe^3+. What is the molarity of the KMnO4 solution?
Write the correct molecular equation, complete ionic equation, and net ionic equation for the reaction between cobalt (II) chloride and hydrocyanic acid. Mention the spectator ions, the state (s, l, aq, g) of the reactants and products and the solubility rules you used to predict the reaction.
Write the net ionic equation for the following molecular equation. MnBr2 (aq) + (NH,)2CO3 (aq) → MnCO3 (8) + 2NH,Br(aq) (Use the lowest possible coefficients. Be sure to specify states such as (aqg) or (s). If a box is not needed, leave it blank.)
What volume in mL of 0.38 M HBr solution is required to titrate 125mL of a 0.18 M Ca(OH)2 solution? Ca(OH)2(aq) + 2HBr(aq) -> CaBr2(aq) + H2O(I)
Classify the reactions represented by these equations as either single or double placement.
What volume in mL of 0.45 M HBr solution is required to titrate 125mL of a 0.21 M Ca(OH)2 solution? Ca(OH)2(aq) + 2HBr(aq) -> CaBr2(aq) + 2H2O(I)
A sample of a chloride salt weighing 484.6 mg is titrated with AgNO3 using K2CrO4 as indicator. To reach the end point a 52.3 mL of 0.1475 M of AgNO3 solution is required. The net ionic equation for the reaction of titration is: Ag+ (aq) + Cℓ- (aq) → AgCℓ (s) How many moles of Ag+ (aq) ions are used to reach the end point? How many moles of Cℓ- (aq) have reacted in the titration? How many grams of chloride are present in the sample? What is the mass percent of chloride in the sample?