04_Ions_PostLab_Spr24

The pH range of a solution can also be determined using indicators. Indicators are molecules that exhibit different colors over a specific pH range. Examples of indicators and the associated colors are shown below. pH Range and Colors 1 2 3 Indicator 4 6 7 Bromcresol green |Congo Red Methyl Yellow Thymol Blue Methyl Violet pH Range and Colors Indicator 2 3 4 5 7 Bromcresol green yellow Oblue Congo Red Methyl Yellow Thymol Blue Methyl Violet Jorange-red Dyellow Dyellow blue red red yellow Oviolet Bromcresol green, for example, would be green between pH 4-5, and gradually change to blue

How do you determine which side the reaction favors in acid base equilibrium problems such as this one?  Subject: Organix Chemistry

Pls help ASAP. Pls do all asked questions.

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1 Initial (M) Change (M) Equilibrium (M) -9 -2.50 × 10-⁹ up for additional resources Determine the Kb for a base by constructing an ICE table and using this information to construct and solve the equilibrium constant expression. Complete Parts 1-2 before submitting your answer. The pH for a 0.0160 M solution of CH3C6H4NH₂ is 8.600. Fill in the ICE table with the appropriate value for each involved species to determine the unknown concentrations of all reactants and products. 0 CH3C6H4NH₂(aq) 100 3.98 x 10-6 1 0.0160 Question 21 of 26 -3.98 x 10-6 + 10 8.60 H₂O(l) 5.4 -8.60 2 -5.4 OH (aq) JU 0.93 NEXT > -0.93 + CH3C6H4NH3(aq) ✓ RESET -9 2.50 x 10-⁹

In this lab the pH was …       measured by litmus paper.     measured by pH paper.     measured by indicators which are sensitive to pH.     measured by a pH meter.

In the laboratory, a general chemistry student measured the pH of a 0.354 M aqueous solution of caffeine, C;H1,N,0, to be 12.063. Use the information she obtained to determine the K, for this base. K„(experiment)

Fill in the left side of this equilibrium constant equation for the reaction of dimethylamine ((CH, ), NH), a weak base, with water. D= K, Explanation Check O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy C へ 80 F Cloudy DELL De F12 PrtScr Insert F9 F10 F11 F8 口

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When is it safe to assume that the change from initial concentration (+/- x) is small enough to be negligible/ignore when doing equilibrium calculations for weak acids and bases? Be specific!

Solve Question 18

Some NH4Cl dissolves in water and is under equilibrium. What is the effect to pump NH3 (g) into the above NH4Cl solution? The process will not change the solution volume. (Choose one option only.) Options: a. The amount of NH4+ will decrease, and the solution pH will increase. b. The amount of NH4+ will decrease, and the solution pH will decrease. c. The amount of NH4+ will increase, and the solution pH will decrease. d. The amount of NH4+ will increase, and the solution pH will increase. e. Adding NH3 into the solution has no effect on the solution pH.

Write the equilibrium-constant expressions and obtain numerical values for each constant in a. the basic dissociation of ethyl amine, C2H5NH2. b. the acidic dissociation of hydrogen cyanide, HCN. c. the acidic dissociation of pyridine hydrochloride, C5H5NHC1. d. the basic dissociation of NaCN. e. the dissociation of H3ASO4 to H³O* and AsO,- f. the reaction of CO;2- with H2O to give H2C03and OH-

please correct name for #9

Calculate the pH after 0.15 mole of NaOH is added to 1.09 L of a solution that is 0.49 M HF and 1.05 M NaF, and calculate the pH after 0.30 mole of HCl is added to 1.09 L of the same solution of HF and NaF. 0.15 mole of NaOH 0.30 mole of HCI

1. The beakers below contain an aqueous solution of three different acids, HX, HY, and HZ, respectively, and represent the solutions at equilibrium. The initial concentrations of all three solutions were the same. Assume the volume of each solution is the same. HX = 00 HY = O0 HZ = 00 H,o'= H,o = H,o'= Answer the following questions. Briefly explain your answers. a. The conjugate base particles are left out of each figure. Draw the appropriate number of conjugate base particles in each beaker above, matching the legend provided for the acid in each beaker. Write the dissociation equation of an acid (HA) in water.

Please help me answer these following

19. Write the formula for the conjugate acid of each of the following. (Omit states-of-matter from your answer.) 20. Write the formula for the conjugate base of each of the following. (Omit states-of-matter from your answer.)

A Bronsted-Lowry acid is converted into its conjugate base by a) accepting a neutron. b) accepting an OH- ion. c) losing a proton (H+). d) accepting a proton (H+). 12:15 PM 4/22/2021 PrtSc Insert Delete 144 F9 F10 FIL F12 Backspace Num Lock 9. 8. Home POUp Enter 2 Shift End Cir LO + I|

5. Calculate the pH and pOH of Aniline and Methylamine if both solutions have a concentration of 0.315 M. Compare the basicity of the two solutions. Write the dissociation equations and expressions. Aqueous-Equilibrium Constants TABLE 2 Dissociation Constants for Bases at 25°C Name Formula NH, CHNH, (CH) NH C,H,NH, HNNH, HONH, CHNH, CHN (ČH)N 1.8 x 10-5 4.3 x 10-10 5.4 x 10-4 6.4 x 10-4 1.3 x 10-6 1.1 x 10- 4.4 x 10-4 1.7 x 10-9 6.4 x 10-5 Amm onia Aniline Dimethylamine Ethylam ine Hydrazine Hydroxylamine Methylamine Pyridine Trimethy lamine Source: https://wps.prenhall.com/