a) Label each species as an Bronsted-Lowry acid or base. Show the conjugate acid-base pairs. HCO; + H;O* H¿CO; + H¿O (aqueous solution) b) Phenol (HC&Hs0) is a weak acid (K,= 1.5 x 104). Write the equilibrium chemical equation, equilibrium constant expression, and calculate the pH of a 0.25 M solution of phenol. 9)

What H 3O + concentration corresponds to each pH value: (a) 13; (b) 7; (c) 3? Label each solution as acidic, basic, or neutral.

Consider the following data on some weak acids and weak bases: acid base Ka K, name formula name formula -4 hydrofluoric acid HF 6.8 × 10 ethylamine C2H;NH, 6.4 × 10 10 4.9 x 10 8. hydrocyanic acid HCN hydroxylamine HONH, 1.1 x 10 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 HONH3CI choose one 0.1 М KF choose one 0.1 M C2H5NH3Br choose one 0.1 М KBr choose one

1) Write a chemical reaction to show the neutralization of hydriodic acid (HI) by sodium hydroxide (NaOH).   2) Give the pH that corresponds to each solution and classify it as acidic, basic, or neutral: [H3O+] = 0.01 [H3O+] = 10-9 [H3O+] = 10-7 [H3O+] = 10-5   3) What is the [H3O+] concentration in a solution with a pH of 4?

Consider the following data on some weak acids and weak bases: acid base Ка K, name formula name formula 8- 3.0 × 10 - 8 hypochlorous acid HCIO hydroxylamine HONH, 1.1 × 10 -4 6.8 × 10 ethylamine C2H5NH2 | 6.4 × 10 alo -4 hydrofluoric acid HF Ar Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to thể"s 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 М KСІ choose one v 0.1 M KCIO choose one v 0.1 M HONH3Br choose one v 0.1 M NaF choose one v

Stuck on this :(

For the following reaction, the products are favored at equilibrium. Classify each of the reactants and products based on their strength as Bronsted-Lowry acids or bases. (C,H3),NH + HCOOH HCO0" + (C,Hg),NH2* Clear All Stronger Bronsted-Lowry acid (C,H3)2NH Weaker Bronsted-Lowry acid HC00" Stronger Bronsted-Lowry base НСООН (C,H3)2NH,* Weaker Bronsted-Lowry base

Consider the following data on some weak acids and weak bases: acid base Ka name formula name formula HNO, 4.5 x 10 CgH;NH2|4.3 × 10 - 10 -4 nitrous acid aniline 4 -8 hydrofluoric acid HF 6.8 × 10 hydroxylamine HONH, 1.1 x 10 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. solution pH 0.1 M HONH3CI choose one v 0.1 M Nal choose one v 0.1 M KNO2 choose onev 0.1 M NaF choose one v

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 =

Identify it as an acid or base. Write the ionization chemical reaction. Calculate the pH, pOH, [H+] or [OH-] 3.38 105 M HNO3 (assume 100% ionization)