Identify the following reactions as acid-base, precipitation, or redox reactions. 5 Ca(OH)2(aq) + 3PO4(aq) → Ca5OH(PO4)3(s) + 9 OH(aq) -> Give detailed Solution of all reactions, don't give Handwritten answer. Ca(OH)2(s) + 2 CH3COOH(aq) → Ca(CH3COO)2(aq) + 2 H2O(aq) precipitation precipitation 8 H+(aq) + MnO4(aq) + Fe2+(aq) → Mn2+(aq) + Fe3+(aq) + 4 H2O() precipitation 12(s)+2 S2032(aq) → S4062(aq) + 2(aq) redox

Identify the following reactions as acid-base, precipitation, or redox reactions. 5 Ca(OH)2(aq) + 3PO4(aq) → Ca5OH(PO4)3(s) + 9 OH(aq) -> Give detailed Solution of all reactions, don't give Handwritten answer. Ca(OH)2(s) + 2 CH3COOH(aq) → Ca(CH3COO)2(aq) + 2 H2O(aq) precipitation precipitation 8 H+(aq) + MnO4(aq) + Fe2+(aq) → Mn2+(aq) + Fe3+(aq) + 4 H2O() precipitation 12(s)+2 S2032(aq) → S4062(aq) + 2(aq) redox

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

CuBr2(aq)+2KOH(aq)→CuOH2(s)+2KBr(aq).Write the net ionic equation for this reaction.
Explain why the neutralization of any strong acid with any strong base, in dilute aqueous solution, can be represented by the equation, H3O* (aq) + OH (aq) → 2 H2O (1).
A 0.124 M NaOH(aq) solution was used to titrate 20.00 mL of an acetic acid (CH3COOH) solution that has an unknown concentration. The equivalence point is reached after adding 15.34 mL of NaOH(aq). a) Write out the complete balanced equation for the reaction that occurs in this titration. b) How man moles of NaOH were added to the acetic acid solution? c) How many moles of acetic acid were in the original 20.00 mL solution? d) What was the concentration of acetic acid in the orignial 20.00 mL solution?
Write the balanced formula, complete ionic, and net ionic equations for each of thefollowing acid-base reactions.a. HClO4(aq) + Mg(OH)2(s) →b. HCN(aq) + NaOH(aq) →c. HCl(aq) + NaOH(aq) →
Classify each of these reactions. 2 NaOH(aq)+Pb(CI0,),(aq)- → 2 NACIO, (aq)+Pb(OH),($) CH,(g) + 20,(g) → CO,(g) + 2 H,0(1) 2 AGNO, (aq)+Zn(s) • Zn(NO, ),(aq) + 2 Ag(s) HI(aq)+L¡OH(aq) – H,O(1)+Lil(aq) Answer Bank precipitation acid base neutralization redox
For the following reaction, 96.8 grams of perchloric acid (HCIO4) are allowed to react with 26.6 grams of tetraphosphorus decaoxide . perchloric acid (HCIO4) ( aq ) + tetraphosphorus decaoxide ( s )- → phosphoric acid ( aq ) + dichlorine heptaoxide (1) What is the maximum amount of phosphoric acid that can be formed? grams What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams
Give the complete ionic and net ionic equation for the reaction below. Circle the spectator ions. Fe(s) + 2 AgNO3(aq) → 2 Ag(s) + Fe(NO3)2(aq)
Hard water contains magnesium and calcium ions 1Mg2+, Ca2+2, which can precipitate out in hot water pipes and water heaters as carbonates. Write the net ionic equation for this reaction.
Please don't provide handwritten solution
Writing net ionic equations The following chemical reaction takes place in aqueous solution: 2 AgF (aq) + K₂S (aq) → Ag₂S(s)+2 KF (aq) Write the net ionic equation for this reaction. 10 ロ→ロ X 1/5 Ś ? olo 18 Ar
Using solubility rules, predict which compound precipitates in the following reactions. Then balance the chemical equations, writing out the total-ionic equations and net-ionic equations. BaCl2(aq) + (NH4)2CO3(aq) → BaCO3(s) + 2NHẠCI(aq)
The following chemical reaction takes place in aqueous solution: 2 AgF(aq)+ (NH4) CO3(aq) → Ag₂CO3(s)+2 NHÂF(aq) 2 Write the net ionic equation for this reaction.