Q. Reactions and Titration Write out the full, balanced equations for the reaction below, and identify whether it has net ionic equation. a. A solution of sodium cyanide and hydrogen bromide. Full balanced equation: Net ionic equation: Yes/No b. A solution of ammonium sulfate and barium nitrate. Full balanced equation: Net ionic equation: Yes/No c. A solution of sulfuric acid and sodium hydroxide. Full balanced equation:

Q. Reactions and Titration Write out the full, balanced equations for the reaction below, and identify whether it has net ionic equation. a. A solution of sodium cyanide and hydrogen bromide. Full balanced equation: Net ionic equation: Yes/No b. A solution of ammonium sulfate and barium nitrate. Full balanced equation: Net ionic equation: Yes/No c. A solution of sulfuric acid and sodium hydroxide. Full balanced equation:

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter9: Acids, Bases, And Salts

Section: Chapter Questions

Problem 9.99E

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In this experiment, you will determine the amount (percent) of potassium hydrogen phthalate (KHP) that is in an impure sample. You will determine the percent of KHP via titration using NaOH with known molarity. The reaction will follow, KHC8H4O4 (aq) + NaOH (aq) ---------> KNaC8H4O4 (aq) + H2O (l) At the endpoint, the moles of KHP will equal the moles of NaOH. You will use phenolphthalein as the indicator. The endpoint of the reaction will be a light pink solution color. How will you know the reaction is over? About how much KHP will be used in the titration? Which 3 substances go into the 250 mL Erlenmeyer flask for the titration? What is the mole to mole ratio in the reaction of KHP and NaOH? What solution goes into the buret?
In the second titration, the molar mass of an unknown monoprotic acid is calculated. If 0.100 grams of unknown solid are dissolved in water and titrated with 4.68 mL of the NaOH, what is the molar mass of the solid? HINTS: Molar mass is grams / moles. We have grams from the weighed mass, we can calculate moles of acid from the titration. Monoprotic means that it produces 1 H+ per molecule. This means that our moles of NaOH added and moles of acid are the same. You will need to use your concentration of NaOH from the previous question
Specialized cells in the stomach release HCl in order to aid in digestion. If these cells release too much HCl, the excess acid can be neutralized with antacids such as TUMS which contain calcium carbonate in order to avoid discomfort. In order to test commercial antacids, a chemist uses 0.160 M HCl to stimulate the acid concentration in the stomach. First, provide a correctly balanced reaction equation for the reaction between hydrochloric acid and calcium carbonate (note that this reaction produces H2O(l) and CO2(g)). Then show how to determine and calculate the amount of stimulated stomach acid (in mL) that would react completely with one extra strength TUMS tablet which contains 7.50x10^2 mg of calcium carbonate. you must use the factor-label(conversion-factor) method for all conversions. Use significant figures and include units where applicable.
Use floating decimal in your solutions but express all final answers to four (4) decimal places and enclose them in a box. A 3 mL sample of concentrated nitric acid solution is diluted to 150 mL. A 15 mL sample of the diluted solution requires 29.43 mL of a 0.0171 molar solution of potassium hydroxide to be titrated to the equivalence point. Determine the mol per liter of the original nitric acid solution
2KMnO4 (aq) +5H2C2O4 (aq) + 3H2SO4 (aq) > 10CO2 (g) + K2SO4 (aq) +2MnSO4 (aq) + 8H2O (l) 90ml of 0.0150 M KMnO4 solution is mixed with 30 ml of 0.095 M H2C2O4 solution in a medium where there is excess sulfuric acid. Assume 100% yield Calculate the concentration of the following ions or molecules in the final solution a) Mn2+ b) K+ c) MnO4- d)H2C2O4
A pure organic compound has the formula C4H8SOx. A sample of a compound wasdecomposed; the sulfur was converted to sulfate and titrated in a modified version of theadsorption indicator procedure. From the following data, determine the correct formula forthe compound.Given: weight of sample = 12.64 mgBa(ClO4)2 needed for titration = 10.60 mL of 0.0100 M Ba(ClO4)2
The reaction of KOH with HNO2 is presented by the unbalanced chemical reaction below: ___ KOH(aq)+ ___ HNO3 (aq)---> ___ KNO3 (aq)+ ___ H2O(l)Calculate the molar concentration of Nitric acid (HNO2) when 40.5 mL of 0.674 M KOH is required to quench 101.0 mL of Nitric acid over phenolphthalein indicator.
Some sulfuric acid is spilled on a lab bench. It can be neutralized by sprinkling sodium bicarbonate on it and then mopping up the resultant solution. The sodium bicarbonate reacts with sulfuric acid as follows: 2NaHCO3 (s) + H2SO4 (aq) --> Na2SO4 (aq) + 2H2O (l) + 2CO2 (g) Sodium bicarbonate is added until the fizzing due to the formation of CO2 (g) stops. If 27 mL of 6.0 M H2SO4 was spilled, what is the minimum mass of NaHCO3 that must be added to the spill to neutralize the acid?
Consider this reaction H2SO4(aq) +2KOH(aq) ---> H2SO4(aq) ---->K2SO4(aq) +2H2O(l) Determine the volume of 0.205 M KOH solution require to neutralize each sampe of sulfuric acid. a. 35mL of 0.205 M H2SO4 b. 205mL of 0.135 M H2SO4 C. 80 ml of 0.100 M H2SO4
A 0.217 g sample of HgO (molar mass = 217 g/mol) reacts with excess iodide ions according to the reaction show below. Titration of the resulting sample solution requires how many moles of 0.10 M KI to reach the equivalence point? Assume complete reaction. HgO + 4 I- + H2O HgI42- + 2 -OH
This is only one question!!! Using this reactions:1) Na2B4O5(OH)4⋅8 H2O (s) → 2 Na+ (aq) + B4O5(OH)42– (aq) + 8 H2O (l) and 2) B4O5(OH)42– (aq) + 2 H3O+ (aq) + H2O (l) → 4 H3BO3 (aq) Using Titration data and the volume of sample. Calculate concentration of Sodium ion in each of the 5 samples: K = [Na+]2[ B4O5(OH)42–] Molarity of HCL 0.2021 Data:40 mL Borox+0.80mL DI water mixed in Erlenmeyer flask, was placed into 1 L beaker and heated to 55C. Then cooled to 50,40.30, 20, and 10 degrees C. Samples Data: Sample Tubes at 50C, 40C, 30C, 20C, 10C 50 degree C = 9.4 ml 40 degree C= 8,60 ml 30C=9.3 ml 20C=9.1ml 10C=3.6 ml Titration data: Titrated with HCL and indicator Bromocresol Green 1) 50 degrees C Initial volume in the burette 0.0 and the color changed to green at 39.10 2) 40 degrees C Initial volume in the burette 0. 00 Color changed at 27.00 ml 3) 30 degrees C tube Initial volume in the burette 0.00 Color changed at 24.40 mL 4) 20 degrees C tube Initial volume in the burette 0.00 Color…
Identify the type of each of the following reactions. 1. N2(g)+2O2(g)→2NO2(g) -- 2. CaCl2(aq)+2AgNO3(aq)→2AgCl(s)+Ca(NO3)2(aq) -- 3 .CS2(l)+3O2(g)→2SO2(g)+CO2(g) -- 4. H3PO4(aq)+3KOH(aq)→3H2O(l)+K3PO4(aq)-- options for each : --precipitation, acid-base, oxidation-reduction, or no reaction