### Precipitation Reaction: Complete Ionic Equation**Given Reaction:**\[ \text{K}_2\text{CO}_3 \text{(aq)} + 2\text{CuF} \text{(aq)} \rightarrow \text{Cu}_2\text{CO}_3\text{(s)} + 2\text{KF} \text{(aq)} \]**Objective:**Write the balanced complete ionic equation for the precipitation reaction shown.**Instructions:**- Express your answer as a chemical equation including phases.- Use an underscore (_) or a caret (^) to add subscripts and superscripts quickly.**Input Area:**In the provided input box, you have the option to use symbols and insert math elements to write out the chemical equation.**Incorrect Submission Notice:**The previously submitted ionic equation was incorrect. Ensure to check your coefficients and charges. You have 5 attempts remaining to submit the correct answer.**Available Tools:**- Mathematical expression symbols for accurate representation.- Superscript and subscript buttons to ensure correct ion notation.For more assistance, you can view the available hints to guide you in constructing the balanced equation.

General equation is – K2CO3aq + 2CuF aq →Cu2CO3s + 2KFaqBalanced ionic equation is – Complete balanced ionic equation-2K+aq + CO32-aq + 2Cu+aq + 2F-aq →Cu2CO3s + 2K+aq +2F-aqNet balanced ionic equation - CO32-aq + 2Cu+aq →Cu2CO3s

Science

Chemistry

K2CO3(aq) + 2CUF(aq) → Cu2CO3(s) + 2KF(aq) The molecular equation you determined in Part B is shown above for your convenience. Examine each of the chemical species involved to determine the ions that would be present in solution. Be sure to consider both the coefficients and subscripts of the molecular equation, and then write this precipitation reaction in the form of a balanced complete ionic equation. Express your answer as a chemical equation including phases. Type an underscore (_) or a carat (^) to add subscripts and superscripts more quickly. • View Available Hint(s) ΑΣφ ? xª b +CO3 2+ →Cu,CO3(9) (aq) (aq) Submit Previous Answers

K2CO3(aq) + 2CUF(aq) → Cu2CO3(s) + 2KF(aq) The molecular equation you determined in Part B is shown above for your convenience. Examine each of the chemical species involved to determine the ions that would be present in solution. Be sure to consider both the coefficients and subscripts of the molecular equation, and then write this precipitation reaction in the form of a balanced complete ionic equation. Express your answer as a chemical equation including phases. Type an underscore (_) or a carat (^) to add subscripts and superscripts more quickly. • View Available Hint(s) ΑΣφ ? xª b +CO3 2+ →Cu,CO3(9) (aq) (aq) Submit Previous Answers

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

Write the net ionic equation for the following molecular equation. HCl is a strong electrolyte. HF is a weak electrolyte. NaF(aq) + HCl(aq) → NaCl(aq) + HF(aq) (Use the lowest possible coefficients. Be sure to specify states such as (ag) or (s). If a box is not needed, leave it blank.)
Write the net ionic equation for the following molecular equation. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.)
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)
How many grams of Cu(OH)2 will precipitate when excess KOH solution is added to 69.0 mL of 0.584 M CuCl2 solution? CuCl2(aq)+2KOH(aq) → Cu(OH)2 (s) + 2KCl(aq) g
Write the balanced precipitation reactions
A student combined CuCl2 (aq) and Na (s). The student observed a color change, thus a reaction occurred. Write the balanced molecular equation for this reaction showing coefficients and phase labels. Write the complete ionic equation for this reaction. Write the net ionic equation for this reaction. Assign oxidation numbers to the reactants and products in the net ionic equation. Which reactant, CuCl2 (aq) or Na (s), got oxidized? Which reactant, CuCl2 (aq) or Na (s), got reduced? Which reactant, CuCl2 (aq) or Na (s), is the oxidizing agent? Which reactant, CuCl2 (aq) or Na (s), is the reducing agent?
A solution of NaCl(aq)NaCl(aq) is added slowly to a solution of lead nitrate, Pb(NO3)2(aq)Pb(NO3)2(aq), until no further precipitation occurs. The precipitate is collected by filtration, dried, and weighed. A total of 10.41 g PbCl2(s)10.41 g PbCl2(s) is obtained from 200.0 mL200.0 mL of the original solution. Calculate the molarity of the Pb(NO3)2(aq)Pb(NO3)2(aq) solution.
Copper (II) chloride, CuCl2(aq) solution is reacted with aluminum hydroxide, Al(OH)3(aq) solution. Write the TOTAL IONIC EQUATION for this reaction.
Consider the chemical reaction. 3 MgCl₂ (aq) + 2 Na₂PO₂ (aq) → Mg3(PO4)₂ (s) + 6 NaCl(aq) Write the net ionic equation for the chemical reaction, including phases.
A solution of NaCl(aq) is added slowly to a solution of lead nitrate, Pb(NO3)2(aq), until no further precipitation occurs. The precipitate is collected by filtration, dried, and weighed. A total of 17.07 g PbCl2(s) is obtained from 200.0 mL of the original solution. Calculate the molarity of the Pb(NO3)2(aq) solution.
How can we calculate the molarity of the solution?
Please don't provide handwritten solution