please help on questions 4,5,6 al and Procedure for each activity A-D. Write a brief (one- or two-sentence) description oftivity B, the effect of concentration on equilibrium will be investigated for the formation ofderately toxic by ingestion. Iron(II) nitrate solution may be a skin/tissue irritant. Concentrated= ingestion or inhalation and is severely corrosive to skin and eyes; can cause severe body tis-diately in case of an acid spill. Dilute hydrochloric acid and sodium hydroxide solutions areocyanate is toxic by ingestion and emits a toxic gas if strongly heated-do not heat this solu-osphate monobasic is moderately toxic by ingestion. Wear chemical splash goggles, chemical-istant apron. Wash hands thoroughly with soap and water before leaving the lab.briumwill be used to study the nature of equilibrium. An indicator is a dye that can gain or loseat have different colors. Equation 2 summarizes the reversible reaction of the indicator brom-uncharged indicator molecule and In- an indicator anion formed after the molecule has lost ae, we can employ LeChâtlier's Principle to predict how equilibrium can be restored: "If anstress, the system will react in such a way as to reduce the stress." The color of the indicatoror OH- ions will show how changing the concentration of a product affects the equilibriumHIn(aq) H*(aq) + In (aq)Color AColor BH*(aq) + OH-(aq) → H₂O(1)04%, 1 mL2 mLOH, 0.1 M, 2 mLBeral-type pipets, graduated, 4Test tube, smallTest tube rackWash bottleEquation 2Equation 3resol Greenin the test tube. Add 5 drops of 0.04% bromcresol green. Swirl gently and record the color N2. Add 3 drops of 0.1 M HCI solution to the test tube. Swirl gently and record the new color of the solution in the data table.3. Add 0.1 M NaOH dropwise to the solution until the original color is restored. Shake gently and record the number of dropsof NaOH added and the color of the solution in the data table.4. Continue adding 0.1 M NaOH dropwise until a total of 5 drops of NaOH have been added in steps 3 and 4 combined.Can the process be reversed to obtain a color that is intermediate between that in steps 2 and 3?5. Add 0.1 M HCl again dropwise very slowly until the solution reaches a "transition" color midway between the twocolors recorded above (steps 2 and 3). Swirl gently between drops to avoid overshooting the transition color. Recordthe number of drops of HCl required and the color in the data table. Note: It may be necessary to add half a dropat a time.6. Wash the contents of the test tube down the drain with excess water and rinse the test tubes with distilled or deionized water.Data TableAcid-Base Equilibrium of Bromcresol GreenInitial color of indicator solution (step 1)Color after addition of HCI (step 2)Color after addition of NaOH (step 3)Number of drops of NaOH added (step 3)Amount of HCl required to obtain "transition" color (step 5)Transition color (step 5)day light bluegolddeep aqua blued. 10 dropromue9 dropsgrevenObservations and Analysis1. Write the chemical equation for the reversible reaction of bromcresol green (HIn) with water. Label this Equation A.2. Use the color changes observed for the indicator before and after adding HCl (steps 1 and 2) to predict the colors of theHIn and In- forms of bromcresol green. Write the colors of HIn and In- underneath their formulas in Equation A. Explainyour reasoning. Hint: Adding HCI increases the concentration of H+ ions. Which reaction, forward or reverse, would thatincrease?3. Explain the observed color change: Adding more product to an equilibrium mixture of reactants and products increases therate of the (forward/reverse) reaction and thus (increases/decreases) the amount of product.4. In step 3, hydroxide ions reacted with and removed H+ ions from solution (see Equation 3). What color change wasobserved when NaOH was added? Which substance (HIn or In) increased in concentration as a result?5. Explain the observed color change: Removing one of the products from an equilibrium mixture of reactants and productsdecreases the rate of the (forward/reverse) reaction and thus (increases/decreases) the amount of product.6. What form(s) of the indicator were most likely present when the transition color was observed in step 5? How does thisobservation provide visual evidence that not all reactions "go to completion?"

The general reaction involved is HIn (aq) <-----> H+ (aq) + In- (aq) The indicator used is…

Answered: 1. In step 3, hydroxide ions reacted…

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...