Given the following information:hypochlorousКа=HCIOacid3.5x10-8benzoic acidC6H5COOHKa =Ка6.3x10-5(1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.368 M aqueous hypochlorous acid and sodiumbenzoate are mixed. It is not necessary to include states such as (aq) or (s).(2) At equilibrium thewill be favored.(3) The pH of the resulting solution will be+seven.+

(1) Net Ionic Equation for the ReactionHypochlorous acid is a weak acid and dissociates in water as…

Answered: Given the following information:…

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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Complete the followin reaction by providing the products formed. Then balance the reaction and write the molecular reaction and the total and net ionic reactions. The reaction is: Zn(NO3)2 (aq) + Ba(OH)2 (aq) ---> Products.
One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe(s)+CuSO4(aq) ----------> Cu(s)+FeSO4(aq) Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 500.mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 104.mg.Calculate the original concentration of copper(II) sulfate in the sample. Round your answer to 3 significant digits. _______________g/L
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.
Given the following information: acetylsalicylic acid (aspirin) hydrocyanic acid (2) At equilibrium the HC₂H704 HCN Submit Answer (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.536 M aqueous acetylsalicylic acid (aspirin) and sodium cyanide are mixed. It is not necessary to include states such as (aq) or (s). (3) The pH of the resulting solution will be will be favored. = Try Another Version Ka = 3.0x10-4 Ka = 4.0x10 10 seven. + 2 item attempts remaining
Sodium hydrogen carbonate (NaHCO3), also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HC1), which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl(aq) + NaHCO3(aq) - NaCl(aq) + H₂O(l) + CO₂(g) The CO₂ gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 100. mL of a 0.011 M HCl solution. What mass of NaHCO3 would he need to ingest to neutralize this much HCl ? Round your answer to 2 significant digits. 6.D x10 X Ś
Sodium hydrogen carbonate (NaHCO,), also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HCI) , which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO, neutralizes excess HCl through this reaction: HCl(aq) + NaHCO3(aq) → NaCl(aq) + H,O(1) + CO,(9) The CO, gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 150. mL of a 0.049 M HCl solution. What mass of NaHCO, would he need to ingest to neutralize this much HCl ? Be sure your answer has the correct number of significant digits.
Write the net ionic reaction for the following double replacement reaction.
For the reaction of the precipitation of sulfate ions in water as BaSO4;a) Write the net ionic equation.b) What is the initial sulphate ion concentration since 0.320 g BaSO4 is precipitated as a result of the treatment with excessive amount of BaCl2 for 3500 ml of water? (Ba = 137.3 g / mol, O = 16.0 g / mol, S = 32.0g / mol, Cl = 35.45 g / mol)
The concentration of Sn²+ in a solution is determined by titrating it with a 0.1890 M permanganate solution. The balanced net ionic equation for the reaction is: 2MnOq°(aq) + 5Sn²*(aq) + 16H3O*(aq) → 2Mn²+(aq) + 5Sn*(aq) + 24H,O(1) In one experiment, 24.99 mL of the 0.1890-M permanganate solution is required to react completely with 40.00 mL of the Sn2+ solution. Calculate the concentration of the Sn2+ solution. M
Malic acid (C4H6O5) is a dicarboxylic acid that naturally occurs in the production of bignay wine. Maria was tasked to find out the acid content in a 200.0 mL wine sample by titrating it with a standardized solution of KOH. He was able to establish the working concentration of the KOH solution by using 39.12 mL of it to titrate a primary standard of KHP that weighed 3.021 g. The grams and %w/w of Malic acid present in the 200.0 mL wine sample were then determined by titrating a 20.00 mL aliquot using 48.95 mL of the standardized KOH solution. C4H6O5 (aq) + 2KOH (aq) ↔ K2C4H4O5 (aq) + 2H2O (l) Assume the density of the wine sample is 1.000 g/mL MM of KHP = 204.22 g/mol MM of C4H6O5 = 134.0874 g/mol What is the molar concentration of the prepared KOH solution?…
Classifiy each by key reaction event (Precipitation, Acid/Base, Redox) and changes in composition (Combination, Decomposition, Single Displacement Reaction, Single Displacement Reaction). 2NaHCO3(aq) + H2SO4(aq) --> 2CO2(g) + 2H2O(l) + Na2SO4(aq) 2ClO(g) + H2(g) ---> HCl(g) + 4H2O(g)
Sodium hydrogen carbonate NaHCO3, also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl, which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl(aq)+NaHCO3(aq)→NaCl(aq)+H2O(l)+CO2(g) The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a woman suffering from indigestion can be considered to be 200.mL of a 0.089M HCl solution. What mass of NaHCO3 would she need to ingest to neutralize this much HCl? Be sure your answer has the correct number of significant digits.

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