No Plagiarism Please! Use the "My solution mode" simulation to complete Describe how you could adjust the settings of the simulation to increase the number of red (H3O+) and blue (A-) particles in the solution of equilibrium. In three to four sentences, justify your answer and explain how and why this would change the pH of the solution. https://phet.colorado.edu/sims/html/acid-base-solutions/latest/acid-base-solutions_en.html

No Plagiarism Please! Use the "My solution mode" simulation to complete Describe how you could adjust the settings of the simulation to increase the number of red (H3O+) and blue (A-) particles in the solution of equilibrium. In three to four sentences, justify your answer and explain how and why this would change the pH of the solution. https://phet.colorado.edu/sims/html/acid-base-solutions/latest/acid-base-solutions_en.html

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter5: Equilibrium, Activity And Solving Equations

Section: Chapter Questions

Problem 5P

See similar textbooks

Similar questions

Nitrous acid (HNO2) is an essentially nonvolatile acid that ionizes in water with an equilibrium constant of 4 x 10-4 mol/liter. Assume that 10 mmol of nitrous acid are added to a liter of water that is open to the atmosphere.a. List all chemical species that you expect to occur in the water. For which of these do you know the concentration a priori? (you may assume the water has reached equilibrium with the air, and therefore H2CO3* concentration is approximately 12 mM, per Henry’s law)b. Write every equation that constrains the composition of the system at equilibrium identifying each as a mass conservation, mass action, or electroneutrality constraint.
Q1.0 When 0.39 mol of solid CO2 is reacted with 0.23 mol of CH3MgBr in an ether solvent, the resulting product is isolated in aqueous solution (assuming 100% yield) and any excess CO2 is removed. Following this, 0.13 mol of HCl (aq) is added. What is the resulting solution's pH? Please note that you will need to research a pKa value for this query, and your answer should be reported to two decimal points.
A solution of sodium acetate is prepared using 0.56 mol L-1 NaOH as the solvent. The pKapKa of acetic acid is 4.75 . The concentration of sodium acetate after mixing, before any reaction takes place is 0.44 mol L-1 . Calculate the equilibrium concentrations of all acid species: [ CH3COOH ], [ CH3COO- ], the pH and the pOH in the solution. Some assumptions may not work, on the other hand, if you do not make the correct assumptions first, the quadratic formula will give you the wrong answer. [ CH3COOH ] = ___mol L-1 , [ CH3COO- ] = ___mol L-1 , pH = ___ pOH = ____
please help me answer a nad then b a. In the laboratory, a general chemistry student measured the pH of a 0.590 M aqueous solution of ethylamine, C2H5NH2 to be 12.185. Use the information she obtained to determine the Kb for this base. Kb(experiment) =______ b. Now, Write the Ka expression for an aqueous solution of nitrous acid: (Note that either the numerator or denominator may contain more than one chemical species. Enter the complete numerator in the top box and the complete denominator in the bottom box. Remember to write the hydronium ion out as , and not as ) Ka =
Write the dissociation equation for c2h2o4 (acid or base), write the expression for the constant equilibrium according to the law of mass action for c2h2o4, from pKa calculate the value of Ka and Kb for c2h2o4
Determine the pH and concentration of all species at equilibrium for the basic 5-fluorouracil species (C4HFN2O22-). Justify the use of approximations if necessary.Provide the equation for the mass balance of this solution. C4HFN2O22-= 0.30 M
You have a 0.2 M solution of NITROUS acid. Based on references, the ionization constant (Ka) of the said acid at normal temperature is 0.0004. Given the scenario, how much of the hydronium ions (in molars) is present in the solution? Please explain how to obtain the answer for this given scenario. Please do a step-by-step discussion of this problem. Kindly refer to the ICE Table (Initial, Change, & Equilibrium) as a format.
Subject: chemistry Watch this video about acid base equilibria and explain to me step by step on whats happening in the video with long and detailed explanation on whats happening and the conclusion https://youtu.be/rCMRTLANh-w
The acid-dissociation constant for benzoic acid (C6H5COOH) is 6.3×10−5. Part A Calculate the equilibrium concentration of H3O+ in the solution if the initial concentration of C6H5COOH is 0.060 M . Express your answer using two significant figures. part B Calculate the equilibrium concentration of C6H5COO−C6H5COO− in the solution if the initial concentration of C6H5COOHC6H5COOH is 0.060 MM . Express your answer using two significant figures.
Complete the following: 1. Random error, also called _________arises from the effects of uncontrolled variables in the measurement. 2. The ____________,measures how closely the data are clustered about mean. 3. The chemical equilibrium in which all the reactants and products are in the same phase are called____________. 4. Reaction that go to completion and never proceed in the reverse direction are said to be_____________ 5. The equation for buffer is the__________equation. 6. A ___________solution is one that resists changes in pH when small quantities of an acid or an alkali added to it. 7. __________is the pH of the pure, neutral and polyprotic
A mixture of NaCl, SiO2, and CaCO3 is separated following the procedure given in this experiment. Indicate how each of the following procedural changes would affect the amount of the specified substance recovered. Briefly explain. Hint: Refer to Table 1 for Solubility & Reactivity The recovery of CaCO3 was attempted by adding 3M H2SO4 instead of 3M HCl to the SiO2/CaCO3 residue.
Please answer this NEATLY, COMPLETELY, and CORRECTLY for an UPVOTE. Calculate the concentration of each species at equilibrium and the pH of the following solution by applying a) systematic treatment of equilibrium and b) method of succesive approximation. b. 0.100 M methylamine (CH3NH2) (Kb = 4.35 x 10-4)