### Net Ionic Equation for the Reaction**Chemical Reaction:**\[ 2 \text{AgNO}_3(\text{aq}) + \text{K}_2\text{CO}_3(\text{aq}) \rightarrow \text{Ag}_2\text{CO}_3(\text{s}) + 2 \text{KNO}_3(\text{aq}) \]**Task:**Write the net ionic equation for this reaction.**Explanation:**When writing the net ionic equation, we follow these steps:1. **Write the Balanced Molecular Equation:**\[ 2 \text{AgNO}_3(\text{aq}) + \text{K}_2\text{CO}_3(\text{aq}) \rightarrow \text{Ag}_2\text{CO}_3(\text{s}) + 2 \text{KNO}_3(\text{aq}) \]2. **Dissociate All Strong Electrolytes into Their Ions:** - \( 2 \text{AgNO}_3(\text{aq}) \) dissociates into \( 2 \text{Ag}^+(\text{aq}) + 2 \text{NO}_3^-(\text{aq}) \) - \( \text{K}_2\text{CO}_3(\text{aq}) \) dissociates into \( 2 \text{K}^+(\text{aq}) + \text{CO}_3^{2-}(\text{aq}) \) - \( 2 \text{KNO}_3(\text{aq}) \) dissociates into \( 2 \text{K}^+(\text{aq}) + 2 \text{NO}_3^-(\text{aq}) \)3. **Identify the Spectator Ions:** Spectator ions are those that do not participate in the reaction. They appear unchanged on both the reactant and product sides. - In this case, the spectator ions are \( 2 \text{K}^+ \) and \( 2 \text{NO}_3^- \).4. **Write the Net Ionic Equation:** Remove the spectator ions, and write only the ions and compounds directly involved in the reaction. - The net ionic equation is: \[ 2 \text{Ag}^+(\text{

Answered: Image /qna-images/answer/1662adcb-355f-4b88-9ac2-07f80b22999b.jpg

Answered: The following chemical reaction takes…

The following chemical reaction takes place in aqueous solution: 2 AgNO3(aq)+K₂CO3(aq) - → Ag₂CO3(s)+2 KNO3(aq) Write the net ionic equation for this reaction.

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

Complete the balanced neutralization equation for the reaction below: H₂SO₄(aq)+Ca(OH)₂(aq)→
+ Titration of Weak Acid with Strong Base A titration involves adding a reactant of known quantity to a solution of an another reactant while monitoring the equilibrium concentrations. This allows one to determine the concentration of the second reactant. The equation for the reaction of a generic weak acid HA with a strong base is HA (aq) + OH (aq) →A (aq) + H₂O (1) A certain weak acid, HA, with a K, value of 5.61 x 106, is titrated with NaOH. Part A A solution is made by titrating 9.00 mmol (millimoles) of HA and 3.00 mmol of the strong base. What is the resulting pH? Express the pH numerically to two decimal places. ▸ View Available Hint(s) pH = Submit Part B pH = VE ΑΣΦ More strong base added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 42.0 mL ? Express the pH numerically to two decimal places. ▸ View Available Hint(s) IV— ΑΣΦ Submit ? 16 of 3 Review | Constants | Periodic
Using the reaction 2Al(s) + 3CuCl2·2H2O(aq) -> 3Cu(s) + 2AlCl3(aq) + 6H2O(l), complete the oxidation numbers for each element in the table and determine the
Complete the balanced neutralization equation for the reaction below: HC₂H₃O₂(aq)+Sr(OH)₂(aq)→
Chemists working with fluorine and its compounds some- times find it helpful to think in terms of acid-base reac- tions in which the fluoride ion (F¯) is donated and ассеpted. (a) Would the acid in this system be the fluoride donor or fluoride acceptor? (b) Identify the acid and base in each of these reactions: CIF;O2 + BF; CIF,O, · BF, -- TiF, + 2 KF – K2[TiF,]
k= 6.33 × 10−3 L·mol−1·s−1. If the initial concentration of XY is 0.150 mol·L−1, how long will it take for the concentration to decrease to 6.25 × 10−2 mol·L−1 ?
3. Write the products of the reaction between the acid KHP and the base NaOH, and balance the reaction: HKC3H4O4(s) + NaOH(aq) –
If 94.92 mL of a solution of HCl are equivalent to 43.76 mL of a solution of NaOH and if 49.14 mL of the latter will neutralize 0.2162 g of KHC2O4 · H2C2O4 · H2O. What volume of water should be added to a liter of the acid in order to make it 0.5050 normal?
In an electrolysis of a solution with sodium chloride NaCl(aq), sodium hydroxide is formed NaOH(aq), chlorine gas Cl2(g), and hydrogen gas H2(g), after the reaction equation: 2NaCl(aq) + 2H2O(l) → 2NaOH(aq) + Cl2 (g) + H2(g) a) An electrolysis is a redox reaction. What substance is oxidized, and what substance is reduced in the electrolysis of the solution with sodium chloride NaCl(aq)? Base your answer by showing to change in oxidation figures. b) Use the table at the back of the task set and set up two half-reactions describing what is happening on the anode and cathode of this electrolysis.
The following chemical reaction takes place in aqueous solution: AgNO3(aq) + NH4Br(aq) →AgBr(s)+NH4NO3(aq) Write the net ionic equation for this reaction. 11 ロ→ロ X Ś
The following chemical reaction takes place in aqueous solution: FeBr2(aq)+Na2S(aq)→FeS(s)+2NaBr(aq) Write the net ionic equation for this reaction.
Which reaction(s) can be identified as a redox reaction? CuO(s) + H₂SO4(aq) → CuSO4(aq) + H₂O(1) Cu(NO3)2(aq) + 2NaOH(aq) -> A →→ Cu(OH)₂(s) + 2NaNO3(aq) Cu(OH)2(s) CuO(s) + H₂O(g) CuSO4(aq) +Zn(s) → ZnSO4(aq) + Cu(s) Cu(s)+ 4HNO3(aq) - Cu(NO3)2(aq) + 2NO₂(aq) + 2H₂O(1)