10. Write a molecular, ionic and net ionic equation for the reaction between acetic acid (CH3COOH) andsodium hydroxide.Hint: Acetic acid does not lose its hydrogen when dissolved in water so write CH3COOH(aq) foracetic acid in all the equations below. However, it can lose the hydrogen when a OH ion reacts withit to form water so you will need to write Nat (aq) + CH3COO (aq) for NaCH3COOH in the ionicequation and take that into account when determining the net ionic equation.Molecular Equationlonic EquationNet lonic Equation

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Answered: 10. Write a molecular, ionic and net…

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...

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You have an aqueous solution containing one or more of the following anions CO3*, cr, r and SO4. When you add Ba(NO)3(aq) you get a precipitate. You separate the precipitate (A) from the supernatant (B). To the precipitate (A), you add HCI(aq) and the solution fizzes and produces a colorless, odorless gas. To the supernatant (B), you add Ag(NO)3 and there is no reaction. Identify which ions are present, might be present, or are not present Co32- A. present B. not present CI C. might be present Soą2-
For the reaction Ba(OH)2 (aq) + (NH4)½CO3 (aq)--> What one of the following species would appear in the molecular equation? (Don't worry about coefficients. Just write the molecular equation, and see which of these appears in it.) OH (s) Ba2 (aq) O NH,OH (s) BaCO3 (s) O NH2"(aq)
Three acid samples are prepared for titration by 0.03 M NaOH: Sample 1 is prepared by dissolving 0.03 mol of HCl in 20 mL of water. Sample 2 is prepared by dissolving 0.03 mol of HCl in 30 mL of water. Sample 3 is prepared by dissolving 0.03 mol of HCl in 40 mL of water. a Without performing a formal calculation, compare the concentrations of the three acid samples (rank them from highest to lowest). O3>2>1 O1>3> 2 O3>1> 2 O2>1>3 O1>2>3 O2>3>1 Submit Submit Answer Try Another Version 6 item attempts remaining
Write the correct molecular equation, complete ionic equation, and net ionic equation for the reaction between cobalt (II) chloride and hydrocyanic acid. Mention the spectator ions, the state (s, l, aq, g) of the reactants and products and the solubility rules you used to predict the reaction.
17. Predict whether or not a precipitation reaction will occur if the pairs of solutions that are given below are mixed. If you think a reaction will occur, write a balanced equation for the precipitation reaction. Na,S0,(aq) + K2CO3(aq)→ К,со, (аq) + Са(NO;3)2(aq) > СаCl2(aq) + NaNO3(аq) — СаCl2(aq) + 2AgNO,(aq) —
4. Calculate the calculate the mass of precipitate formed from 5.0 g of strontium chloride. Li3PO4(aq) → Sr3(PO4)2(S) + LiCl(aq) _SrCl₂(aq) + 5. What mass of aluminum hydroxide in needed to neutralize 5.00 g of hydrochloric acid? Al(OH)3(s) + _HCl(aq) → ___AlCl3(aq) + _H₂O(1) 195
A reaction is carried out by mixing together a solution of HF and a solution of NaOH. HF (aq) + NaOн (аq) —> н,О (1) Assume the purple particles below each represent 1 mole of particles. Construct the balanced net ionic equation by dragging the purple components into the gray boxes. Drag each unreacted spectator ion along with its balancing coefficient into the blue box that represents the aqueous solution. Remember when you identify spectator ions to look carefully at what changes chemically! + NaF (aq)
The reaction of hypothetical elements: A, B, C, D, and E, follows the molecular equation: AB2(aq) + CDE(aq) -> AE(s) + CB(aq) + DB(aq) Assuming that all aqueous compounds would fully dissociate, indicate the element/s that would form spectator ions in the subsequent total ionic equation.
I understand the concept of the net ionic equation but I don’t understand this example.
Strong acid-base reactions are a subcategory of double displacement reactions. The hydrogen ion of the acid "switches places" with the cation of the base, while the hydroxide ion of the base "switches places" with the anion of the acid. 1. Write the correct product(s) of the following reaction. Include physical states! Also balance the chemical reaction by writing correct coefficients. NaOH(aq) + HCl(aq) 2. Write the correct product(s) of the following reaction. Include physical states! Also balance the chemical reaction by writing correct coefficients. _NaOH(aq) + H SO (aq) 3. Suppose it takes 10 mL of 0.1 M HCl to neutralize 10 mL of 0.1 M NAOH. (“M" = molarity, which is a unit of concentration.) How many milliliters of 0.1 M H,SO, do you expect will be needed to neutralize 10 mL of 0.1 M NaOH? Explain your choice.
This question has multiple parts. Work all the parts to get the most points. Complete and balance the equation for the following acid-base reaction. Name the reactants. Assume complete neutralization. (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (ag) or (s). If a box is not needed, leave it blanl H3 AsO4 (aq) + NaOH(aq) → |H3 AsO4 (aq) + NaOH(aq)
[References] Write net ionic equations for the following molecular equations. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank. Use H for hydronium ion.) HBr(aq) + NH3 (aq) NH, Br(aq) a. 2HI(ag) + Ba(OH)2(ag) → 2H,0(1) + Bal2 (aq) +. C. Pb(NO3)2(ag) + 2NAB1(ag) → PbBr2 (s) + 2NaN03(aq) d. MGCO3 (s) + H2SO4(aq) → MgSO, (aq) + H2O(1) + CO2 (g) b.

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