Conside V following data on some weak acids and weak bases: acid base K. K, name formula formula name hypochlorous acid HCIO 3.0 x 10 C,H,NH, 6.4 × 10 ethylamine -4 acetic acid HCH,CO, 1.8 × 10 hydroxylamine HONH, 1.1 × 10¬8 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution PH 0.1 M KCH3CO2 choose one v 0.1 M C2H5NH3Br choose one 0.1 M NaCIO choose one v 0.1 M KI choose one v

Approximate the final pH of a solution when 1.5 moles of a weak acid is added to water to a final volume of 1L (Ka = 5.67x10^-8). Provide the answer to 3 significant figures.

Consider the following data on some weak acids and weak bases: name nitrous acid acid hydrofluoric acid 0.1 M NaF solution 0.1 M KNO₂ 0.1 M NH4CI 0.1 M C6H5NH3Br formula HNO₂ 4.5× 10 HF Ka X 6.8 × 10 -4 -4 PH Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. choose one choose one choose one choose one S base Kb formula aniline C6H5NH₂ 4.3 x 107 -10 NH3 name ammonia 1.8 x 10 -5

O ACIDS AND BASES Calculating the pH of a weak base solution 0/3 The base protonation constant ₂ of trimethylamine ((CH³)²N) ¡S 6.31×10¯³. Calculate the pH of a 0.27 M solution of trimethylamine at 25 °C. Round your answer to 1 decimal place. pH = 0 X

Complete the table below. Be sure each of your answer entries has the correct number of significant digits. You may assume the temperature is 25 °C. conjugate acid formula HNO₂ HCH, CO₂ Ka 4.5 × 10 -4 -5 1.8 x 10 conjugate base K₂ formula CHONH 0 2.1 10 0- X 3

Be sure to answer all parts. Please report your answer to the correct number of significant figures. Determine the K, of a weak base if a 0.617 M aqueous solution of the base at 25°C has a pH of 10.88. x 10 (Enter your answer in scientific notation.)

Assuming 0.1 M concentrations, arrange the following acid solutions in order of increasing pH. benzoic acid, HC7H5O2, Ka ≡ 6.3 × 10−5 chlorous acid, HClO2, Ka ≡ 1.1 × 10−2 formic acid, HCHO2, Ka ≡ 1.8 × 10−4 hydrofluoric acid, HF, Ka ≡ 6.8 × 10−4

Consider the following data on some weak acids and weak bases: base acid K₁ Kb name formula name formula acetic acid HCH3CO2 1.8 × 10-5 aniline C6H5NH2 4.3 x 10-10 hypochlorous acid HCIO 3.0 × 10 8 hydroxylamine HONH2 1.1 × 10-8 Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. Fynk solution 0.1 M C6H5NH3Br 0.1 M NaCIO 0.1 M HONH3CI 0.1 M KCH3CO2 Check PH choose one choose onev choose one choose one S

The pH of a 0.56M solution of hexanoic acid (HCH0,) is measured to be 2.55. Calculate the acid dissociation constant K, of hexanoic acid. Be sure your answer has the correct number of significant digits. K. = 0 -10 The acid dissociation constant K, of boric acid (H,BO,) is 5.8 x 10 . a Calculate the pH of a 0.42M solution of boric acid. Round your answer to 1 decimal place. pH =

Papaverine hydrochloride (abbreviated papH* CI" ; molar mass 378.85 g/mol) is a drug that belongs to a group of medicines called vasodilators, which cause blood vessels to expand, thereby increasing blood flow. This drug is the conjugate acid of the weak base papaverine (abbreviated pap; K, = 8.33 x 10-9 at 35.0°C). Calculate the pH of a 32.0-mg/mL aqueous dose of papH+ Cl prepared at 35.0°C. Kw at 35.0°C is 2.1 x 10-14. pH =