1. Circle the correct NET ionic equation for the reaction (if any) that occurs when aqueous solutions of K,S andFe(NO,), are mixed.a) K*an) + NO,tag) > KNO34)taa)laa)b) Fe+na) + S,+2 K*1+2 NO,ao)_→ FeS +2 K*la)laa)*tae) + 2 NO,)c) Fe*(aa) + S2,fag) +2 K+12 NO,→ Fe*taa)+S2faa) +2 KNO3)(aallaa)d) Fe*2,laa) + S2(aa)> FeSs)e) No reaction occurs.2. Circle the reagent below that could NOT be used to separate Br* from s? when added to an aqueous solutioncontaining both?a) AgNOles)b) Ca(NO,)z{@e)c) Cu(NO,)2(g)d) Fe(NO;)3{aa)e) All of these.3. In the reaction between AgNO, + HI, the spectator ion(s) would be

A question based on general chemistry that is to be accomplished.

1. Circle the correct NET ionic equation for the reaction (if any) that occurs when aqueous solutions of K;S and Fe(NO,); are mixed. a) Km) + NO,a)→ KNO16) b) Fea) + S, nes + 2 K*ina) + 2 NO;* → FeS + 2 K*na) + 2 NO,*aa) c) Fe* +S, +2 K*iaa) +2 NO,²taal_→ Fe*a) +S², laa) +2 KNO) d) Fe*aa) + Saal > FeS e) No reaction occurs. 2. Circle the reagent below that could NOT be used to separate Br* from S? when added to an aqueous solution containing both? a) AgNOlga) b) Ca(NO,)zto) c) Cu(NO,)x(@s) d) Fe(NO,)\a) e) All of these. 3. In the reaction between AGNO, + HIl, the spectator ion(s) would be

1. Circle the correct NET ionic equation for the reaction (if any) that occurs when aqueous solutions of K;S and Fe(NO,); are mixed. a) Km) + NO,a)→ KNO16) b) Fea) + S, nes + 2 Kina) + 2 NO; → FeS + 2 Kna) + 2 NO,aa) c) Fe* +S, +2 Kiaa) +2 NO,²taal_→ Fea) +S², laa) +2 KNO) d) Feaa) + Saal > FeS e) No reaction occurs. 2. Circle the reagent below that could NOT be used to separate Br from S? when added to an aqueous solution containing both? a) AgNOlga) b) Ca(NO,)zto) c) Cu(NO,)x(@s) d) Fe(NO,)\a) e) All of these. 3. In the reaction between AGNO, + HIl, the spectator ion(s) would be

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...

See similar textbooks

Similar questions

Does a reaction occur when aqueous solutions of cobalt(II) acetate and potassium iodide are combined? O yes O no If a reaction does occur, write the net ionic equation. Use the solubility rules provided in the OWL Preparation Page to determine the solubility of compounds. Be sure to specify states such as (aq) or (s). If a box is not needed leave it blank. +
O SIMPLE REACTIONS Ghaya Determining the volume of base needed to titrate a given mass... A chemistry student weighs out 0.0544 g of acrylic acid (HCH,CHCO,) into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1900 M NAOH solution. Calculate the volume of NAOH solution the student will need to add to reach the equivalence point. Round your answer to 3 significant digits. mL x10 18 Ar Explanation Check © 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use I Privacy Accessibility 7:37 PM ») ENG 2/27/2021 P Type here to search DELL PrtScr Insert Home End Delet Esc F8 F9 F10 F11 F12 F1 F2 F3 F4 F5 F6 F7 # 24 & Back 2 ĭ 3 ř 4{5 0 6 7 7 Y 8 A 9 q o
A solution is prepared by dissolving 2.95 g Co2(SO4)3 in enough water to make 1.00 L of red solution; the red color is due to the presence of the cobalt ions. To this solution was added 1.52 g of magnesium powder. A redox reaction occurred, in which the magnesium atoms lose all of their valence electrons and the red color of the solution fades. (a) Write the total reaction that occurs and the net ionic equation for the redox process. (Assume that one of the products of the redox reaction is a metal.) (b) Calculate the initial concentration of cobalt ions, the final concentration of cobalt ions, and the final concentration of magnesium ions.
49. [Algoríthmíc] A 3.00-g sample of an alloy (containing only Pb and Sn) was dissolved in nitric acid (HNO,). Sulfuric acid was added to this solution, which precipitated 2.93 g of PBSO4. Assuming that all of the lead was precipitated, what is the percentage of Sn in the sample? (molar mass of PbSO = 303.3 g/mol) a) 33.3% Sn b) 17.7% Sn c) 50.0% Sn d) 66.7% Sn e) 2.00% Sn ANS: a) SECTION: 4.7 LEVEL: hard 80 © Houghton Mifflin Company. All rights reserved.
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?
Does a reaction occur when aqueous solutions of sodium carbonate and manganese(II) iodide are combined? O yes no If a reaction does occur, write the net ionic equation. (Use the solubility rules provided in the OWL Preparation Page to determine the solubility of compounds. Be sure to specify states such as (aq) or (s). If a box is not needed leave it blank.) + →
Be sure to specify states such as (aq) or (s). If a box is not needed leave it blank. If no reaction occurs leave all boxes blank and click on "Submit". Use H* for hydronium ion. Write a net ionic equation for the reaction that occurs when potassium sulfite (aq) and excess hydrochloric acid (aq) are combined. Note: Sulfites follow the same solubility trends as sulfates. +
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.)
4. When a solutions of aluminum sulfate and potassium hydroxide are mixed, a precipitate forms. a. Write a balanced net ionic equation for the reaction. b. Calculate the mass of the precipitate when 3.89 g of aluminum sulfate in 100mL of solution is combined with 50 mL of the o.300 M KOH. c. What is the molarity of the ion in excess? (Ignore the spectator ions and assume that volumes are additive)
1. When the following cations and anions react, if the product is insoluble in water, write the net ionic equation for the precipitate reaction.(a) Ag+ and Cl- (b) Ba2+ and SO42- (c) Na+ and Cl-, (d) Zn2+ and NO3-
List the ions and molecules that may have precipitated as part of your final salt product. Step 1. Dissolve the Aluminum metal : (adding solid Al to a Kott Solution) Peaction between Al metal and kot. AICOH and H₂ gas.. Net ionic equation: Solution produces Tetrahydroko aluminate ion 2 A1 (s) + 20H (aq) + 6 +₂0 (1) → 2 Al (OH) - (aq) + 3H2(g) K+(aq) OH(aq) equation that describes the reaction of Sulfuric acid in water: OR H₂SO4 (aq) + H₂0 (1) H₂O+ (aq) + Hs 04" (aq) 2- HSO4 (aq) + H₂O (1) H₂0+ (aq) + 504³ (aq) Step 3: Neutralize base with acid OH reacts with acid: H₂Ocaq) + OH(aq) → 2+1₂0 (1) • Al(OH), reacts with small amount of acid; Alcot)" (q) + Hy" O cag) Al(only (n+ H₂OCD Al(OH) reacts with large amount of acid (with heat): Al (DH), (s) + 3H₂ 0 (aq) → A1 " (aq) + 6 H₂0 (1)
Does a reaction occur when aqueous solutions of zinc sulfate and silver(I) acetate are combined? Oyes no If a reaction does occur, write the net ionic equation. Use the solubility rules provided in the OWL Preparation Page to determine the solubility of compounds. Be sure to specify states such as (aq) or (s). If a box is not needed leave it blank. + ->