Consider the following data on some weak acids and weak bases: acid base K. K, name formula name formula acetic acid HCH;CO2 1.8 x 10-5 ethylamine C,H5NH, 6.4 × 10¬4 hydrocyanic acid HCN C,H;NH2 4.3 × 10¬10 4.9 × 10¬10 aniline 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 C2H5NH3B choose one v 0.1 M C6H5NH3CI choose one v 0.1 M NaCN choose one v 0.1 М КСI choose one v

The pH of a 1.2M solution of hexanoic acid (HC H,,0,) is measured to be 2.39. Calculate the acid dissociation constant K, of hexanoic acid. Be sure your answer has the correct number of significant digits. K a x10

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

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

Calculate the pH of the mixture of 105 mL of 0.195 mol/L hydrazine (H2NNH2) with 95 mL of a 0.215 mol/L H2NNH3Br solutionGive an answer to at least 3 decimal places. Next, calculate the pH of this same solution if 12.00 mL of 0.300 mol/L HNO3 is added.Give an answer with at least 3 decimal places.

The pH of a 0.57M solution of acetic acid (HCH3CO2) is measured to be 2.49. Calculate the acid dissociation constant K of acetic acid. Round your answer to 2 significant digits. K = 0 a x10

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 =

Conside following data on some weak acids and weak bases: acid base K. name formula name formula HNO, 4.5 x 10 aniline C6H3NH, |4.3 × 10 4 - 10 nitrous acid hypochlorous acid HC1O -8- 3.0 × 10 NH3 5 1.8 × 10 ammonia 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 NH4Br choose one ● 0.1 M C6H5NH3CI choose one ● 0.1 M NaCl choose one ● 0.1 М KCIO choose one O

Which is false? O CH3COOH is a weak acid H,PO4: HPO,2 is the principle weak acid/conjugate base pair responsible for maintaining a neutral pH in blood O H,PO4 is both a weak acid and a weak base NAOH is a strong base An amino acid is both a weak acid and a weak base