A 1.00 liter solution contains 0.51 M ammonia and 0.39 M ammonium chloride. If 0.2 moles of hydrochloric acid are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of hydrochloric acid.) _______TrueFalse A. The number of moles of NH3 will remain the same. _______TrueFalse B. The number of moles of NH4+ will remain the same. _______TrueFalse C. The equilibrium concentration of H3O+ will increase. _______TrueFalse D. The pH will remain the same. _______TrueFalse E. The ratio of [NH3] / [NH4+] will increase

A 1.00 liter solution contains 0.51 M ammonia and 0.39 M ammonium chloride. If 0.2 moles of hydrochloric acid are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of hydrochloric acid.) ___TrueFalse A. The number of moles of NH3 will remain the same. _TrueFalse B. The number of moles of NH4+ will remain the same. _TrueFalse C. The equilibrium concentration of H3O+ will increase. _TrueFalse D. The pH will remain the same. _____TrueFalse E. The ratio of [NH3] / [NH4+] will increase

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 100QRT

See similar textbooks

Similar questions

A solution is 0.01F with respect to Mg++ ions. What concentration of hydroxide ions in formula weights per liter will be needed to precipicate Mg(OH)2? The Ksp of Mg(OH)2is 1.2 x10^-11
Using the stock solution concentrations of 0.20 M Fe3+ and 2.0*10^-3 M SCN-, calculate the following concentrations of Fe3+ and SCN- after they have been mixed. (Hint: use the dilution equation M1*V1 = M2*V2) 1. 2ml of Fe3+ and 0.25 ml SCN- 2. 2ml of Fe3+ and 1 ml SCN- 3. 2ml of Fe3+ and 2.25 ml SCN-
Calculate the moles of Cl- ions in 25.0 mL of 0.200 M MgCl2 solution. Group of answer choices 0.0100 mole 10.0 moles 0.00500 mole none of these
A commercial vinegar was analyzed by titration to determine the percent acetic acid. Briefly, 10.00 mL of vinegar sample was diluted to 100. mL solution in a volumetric flask. A 25.00 mL aliquot from the diluted vinegar required 25.55 mL of 0.1005 M sodium hydroxide to reach the phenolphthalein endpoint From this experiment which is the standard solution used in titration? CH3COOH NaOH NaCH3COO C20H14O4
Normality is same as Molarity for sodium hydroxide and normal = molar (for NaOH) Normality of sodium hydroxide = 0.10395N (normal) or Molarity of NaOH = 0.10395M (molar) Volume of NaOH consumed during the titration = 21.87 mL Mol wt of Naproxen = 230.26 g/mol Weight of Naproxen ds (i.e., sample) = 0.534g Calculate the % Purity (dried-basis) of Naproxen ds, given that the LOD results for Naproxen = 1.0% a 97.0 b 98.0 c 98.5 d 99.0 e 99.5 f none of the other answers.
did you get the ppm Cu in the first table?
If you added 1 gram of BaSO4 to 2.5 liters of water, what percentage of the 1 gram would actually dissolve in the water? As a separate problem, if you had another 2.5 liters of pure water and added 25 ml of 2.8 x 10-3 M Na2SO4 as a common ion, what percent of the 1 gram of the BaSO4 would now be able to dissolve?
A 1.00 liter solution contains 0.60 moles nitrous acid and 0.46 moles potassium nitrite .If 0.23 moles of perchloric acid are added to this system, indicate whether the following statements are true or false.(Assume that the volume does not change upon the addition of perchloric acid.) A. The number of moles of HNO2 will increase. B. The number of moles of NO2- will remain the same. C. The equilibrium concentration of H3O+ will remain the same. D. The pH will increase. E. The ratio of [HNO2] / [NO2-] will increase.
A 1.00 liter solution contains 0.36 moles hydrofluoric acid and 0.28 moles sodium fluoride .If 0.14 moles of hydroiodic acid are added to this system, indicate whether the following statements are true or false.(Assume that the volume does not change upon the addition of hydroiodic acid.) A. The number of moles of HF will remain the same. B. The number of moles of F- will decrease. C. The equilibrium concentration of H3O+ will increase. D. The pH will remain the same. E. The ratio of [HF] / [F-] will remain the same.
Moles of NaOH at the equivalence point? Mass of H2C2O4·2H2O= 1.32191 g Volume of the H2C2O4·2H2O solution= 250.0 mL
0.02 M NaOH reagent was standardized using 0.1000 g Potassium hydrogen phthalate (204.22 g/mol) and it required 25.8 mL to reach end point.
Determine the Concentration of Ethanoic Acid in Vinegar Equipment / Apparatus:  250-mL conical flasks  Clamp  Burette  Graduated cylinder  Pipette Reagents / Materials:  Vinegar  Phenolphthalein indicator  0.2 M NaOH (standardized) Calculation: Molarity (M) of ethanoic acid  The average measured volume of the NaOH from titration: Average volume of NaOH used = (21.5ml + 21.5ml + 21.6ml) / 3 =21.5ml No of mole of NaOH = Concentration of NaOH (0.2M) × Average volume of NaOH used When an acid is completely neutralized: No of moles of CH3COOH = No of moles of NaOH Using the moles of CH3COOH, the molarity of ethanoic acid in the 5.0-mL sample of vinegar is calculated: Molarity (M) CH3COOH = moles CH3COOH / volume of vinegar (0.005 dm3). Calculation: Mass / Volume Percent (m/v) of ethanoic acid To calculate the percent (m/v) of CH3COOH in vinegar, we convert the moles of ethanoic acid to grams using the molar mass of ethanoic acid, 60.1 g/mole. Mass of CH3COOH =…