Use the References to access important values if needed for this question.Write the net ionic equation for the following molecular equation.ZnCl2 (aq) +NazCO3(aq)→ ZnCO3(s) + 2NaCl(aq)(Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.)+tps://als-asp.cengage.info/als-asp/takeae Type here to search

Zinc chloride reacts with sodium carbonate to form zinc carbonate and sodium chloride. The equation…

Answered: Write the net ionic equation for the…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 35QRT

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Sodium thiosulfate, Na2S2O3, is used as a fixer in black-and-white photography. Suppose you have a bottle of sodium thiosulfate and want to determine its purity. The thiosulfate ion can be oxidized with I2 according to the balanced, net ionic equation I2(aq) + 2 S2O32(aq) 2 I(aq) + S4O62 (aq) If you use 40.21 mL of 0.246 M I2 in a titration, what is the weight percent of Na2S2O3 in a 3.232-g sample of impure material?
The iron content of hemoglobin is determined by destroying the hemoglobin molecule and producing small water-soluble ions and molecules. The iron in the aqueous solution is reduced to iron(II) ion and then titrated against potassium permanganate. In the titration, iron(ll) is oxidized to iron(III) and permanganate is reduced to manganese(II) ion. A 5.00-g sample of hemoglobin requires 32.3 mL of a 0.002100 M solution of potassium permanganate. The reaction with permanganate ion is MnO4(aq)+8H+(aq)+5Fe2+(aq)Mn2+(aq)+5Fe3+(aq)+4H2O What is the mass percent of iron in hemoglobin?
Aqueous sodium hypochlorite (NaOCl, household bleach) is a strong oxidizing agent that reacts with chromite ion [Cr(OH)4-] in basic aqueous solution to yield chromate ion CrO42- and chloride ion Cl-. The next ionic equation is: ClO- (aq) + Cr(OH)4-(aq) ------> CrO42-(aq) + Cl-(aq) Unbalanced Balance the equation using the method described in section 1 of the Electrochemistry chapter.
The following reaction occurs in basic solution: _ H2O(aq) + _ MnO4–(aq) + _ ClO–(aq) → _ MnO2(s) + _ ClO4–(aq) + _ OH–(aq) When the equation is properly balanced, what is the sum of the lowest whole-number coefficients? a. 9 b. 10 c. 20 d. 12 e. 6
In an oxidation-reduction reaction, 0.0450 mol of aqueous FeSO4 (source of Fe2+) reacts completely with 120.0 mL of an acidified aqueous solution of KMnO4 (source of MnO4-).5Fe2+(aq) + MnO4-(aq) + 8H+(aq) → 5Fe3+(aq) + Mn2+(aq) + 4H2O(ℓ)What is the molarity of the KMnO4 solution?Provide your answer in decimal notation, rounded to the appropriate number of significant figures.
Consider the chemical reaction that takes place between aqueous iron(III) nitrate and aqueous sodium hydroxide. a.) Complete the balanced molecular chemical equation for the reaction below. If no reaction occurs, write NR after the reaction arrow. Be sure to include the proper phases for all species within the reaction. Fe(NO₃)₃(aq) + NaOH(aq) → b.) Write the balanced COMPLETE ionic equation for the reaction. If no precipitation reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction. c.) Write the balanced NET ionic equation for the reaction. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction.
For a precipitation reaction to be useful in a gravimetric analysis, the product of the reaction must be insoluble. Is Kc > 1, < 1, or ≈ 1 for a useful precipitation reaction?
Consider the following reactions. reaction (1): Mn2+(aq) + SO42−(aq) → MnO4−(aq) + H2SO3(aq) in acidic solutionreaction (2): Ni2+(aq) + Cl−(aq) → Ni(s) + ClO−(aq) in basic solutionreaction (3): Mo(s) + N2O4(g) → MoO2(s) + HNO2(aq) in acidic solutionreaction (4): MnO4−(aq) + Cl−(aq) → MnO2(s) + ClO3−(aq) in basic solution Balance each equation under the specified conditions. (Include states-of-matter under the given conditions in your answer.)reaction (1): Mn2+(aq) + SO42−(aq) → MnO4−(aq) + H2SO3(aq) in acidic solution chemPad Help reaction (2): Ni2+(aq) + Cl−(aq) → Ni(s) + ClO−(aq) in basic solution chemPad Help reaction (3): Mo(s) + N2O4(g) → MoO2(s) + HNO2(aq) in acidic solution chemPad Help reaction (4): MnO4−(aq) + Cl−(aq) → MnO2(s) + ClO3−(aq) in basic solution chemPad Help
Given the react side of the total ionic equation for the neutralization reaction of lithium hydroxide (LiOH) with a Hydrochloric acid (HCl), write the total ionic equation (also known as a complete ionic equation) By entering both reacted and the products species, separated by the reaction arrow. Li+(aq)+OH-(aq)+H+(aq)+Cl-(aq)-->? be sure to include the charges are the ionic species and the physical state of all the reactants and products species. Express your answer is a chemical equation.
CHEMISTRY (Please write the complete solution legibly. No long explanation needed. Answer in 2 decimal places. Box the final answer.) Solve the following: a. Calculate the molarity of hydrochloric acid, HCl, in a solution if 25.00 mL of that solution required35.74 mL of 0.1522 M KOH for complete neutralization in a titration. (Answer: 0.2176 M) b. When aqueous solutions of Ba(NO3)2 and K2SO4 are mixed, a precipitate of BaSO4 results. Writethe molecular, ionic, and net ionic equation for this double displacement reaction. c. 8.50 g of copper (II) sulfate pentahydrate, CuSO4∙5H2O, is dissolved in 250 mL of solution. Whatis the molarity of this solution?
An analyst is planning to standardize a 0.200 mol/L NaOH solution for use in neutralization. For this, he chose to standardize the NaOH solution using potassium hydrogen phthalate. (KHC8O4H4, molecular mass 204.22 g mol/L) - Knowing that potassium hydrogen phthalate is a solid, what is the mass of potassium hydrogen phthalate in grams, the analyst should weigh to standardize the NaOH, anticipating spending 15 mL of NaOH solution approximately 0.200 mol/L ? [Answer; m=0.6123 g] NaOH + KHC8O4H4 → KNaC8O4H4 + H2O(Neutralization reaction in standardization) - Why you need to standardize the NaOH solution and why use potassium hydrogen phthalate?
Potassium permanganate solutions used in oxidation-reduction titrations are often standardized against sodium oxalate, Na₂C₂O₄, used as a primary standard. The reaction involved is 5C₂O₄²⁻(aq) + 2MnO₄⁻(aq) + 16 H⁺(aq) → 2Mn²⁺(aq) + 8H₂O(l) + 10CO₂(g) A 0.2452 g sample of sodium oxalate is dissolved in 100 mL of acid solution, and the permanganate solution is added slowly from a buret. The endpoint is reached when 15.85 mL of the permanganate solution has been added. The molar mass of sodium oxalate is 134.00 g/mol. Calculate [MnO₄⁻], the molar concentration of the permanganate solution.

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Write the net ionic equation for the following molecular equation. ZnCl2 (aq) + Na, CO3 (aq) ZnCO3 (s) + 2N2C1(aq) (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.)