Aspirin, also known as acetylsalicylic acid (ASA), Ka= 3.0 x 10-4, is a medication used to reduce pain, fever, or inflammation. The sodium salt has been used for almost a century because it is more soluble than the acid.  What is the pH of a 0.05 M solution of the sodium salt? Show all chemical reactions and all math involved.  Use ASA as structure of the acid.

▼ Part A Calculate the concentrations of NH and NH3 and the pH in a solution prepared by mixing 19.0 g of NaOH and 0.495 L of 1.5 M NH4Cl. Assume that the volume remains constant. Express your answers using two significant figures. Enter your answers numerically separated by a comma. 15. ΑΣΦ [NH ], [NH3] = Submit Part B PH = Submit Request Answer V—| ΑΣΦΑΛΟ Request Answer www. ? Seg ? M

3,6-Dichloro-2-methoxybenzoic acid (dicamba) is a widely used herbicide with the molecular formula C8H6Cl2O3 . The pKa of dicamba is 1.97. A certain water-based herbicide product contains 169 gL−1 of dicamba. Part A What is the pH of the dicamba solution? Express your answer to two decimal places.

1A) Calculate the concentration of C5H5N solution required to provide a pH of 9.29. The Kb of C5H5N is 1.7 × 10-9 at 25°C. 1B) Calculate the mass of C5H5N needed to prepare 2.20 L of the above solution. (Molar mass = 79.10 g/ mol) 2A) The acid-dissociation constant of hydrocyanic acid (HCN) at 25.0°C is 4.9 × 10-10, What is the pH of an aqueous solution of 0.80 M sodium cyanide (NaCN)? 2B) What would be pH of the above solution if NaCN was a strong base? 3A) Write the conjugate base of the following: a) C7H602. b) HCO3- c) ) HASO3²- 3B) Write the conjugate acid of the following: a) PH3 b) SiO32- c) BrO3" 3C) Using 3A-a (C7H6O2) and its conjugate-base as an example, prove that "KąKp = Kw" Search or type URL く=

O ACIDS AND BASES Calculating the pH of a salt solution Calculate the pH at 25 °c of a 0.69M solution of potassium acetate (KCH,CO₂). Note that acetic acid (HCH₂CO₂) is a weak acid with a pà of 4.76. Round your answer to 1 decimal place. pH = 0 1/3 X

A 0.037 M solution of a weak acid (HA) has a pH of 4.59. What is the Ka of the acid? Ka =___×10^__ (Enter your answer in scientific notation.)

A chemist dissolves 617. mg of pure barium hydroxide in enough water to make up 180. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Round your answer to 3 significant decimal places. ☐ x10 G

Calculate the pH of each solution. A solution containing 0.0300 M maleic acid and 0.041 M disodium maleate. The K₂ values for maleic acid are 1.20 × 10-2 (K₁1) and 5.37 × 10-7 (K₁2). pH = A solution containing 0.0248 M succinic acid and 0.014 M potassium hydrogen succinate. The K₂ values for succinic acid are 6.21 x 10-5 (Kal) and 2.31 × 10-6 (K₁2). pH =

Unit 2: Chemical Systems & Equilibrium Butanoic acid, C3H₂COOH, gives rancid butter its distinctive odour. Calculate the pH of 0.020 mol/L solution of butanoic acid. K₂ = 1.51 x 10-5

At a particular temperature, the Ka of benzoic acid (C6H5COOH) is equal to 7.1 x 10-5. What is the pH of a solution prepared by combining 0.479 mol of a the acid with 0.143 mol of C6H5COONa (the sodium salt of the acid) in 4.0 L of water? Report your answer to the hundredths place and do not include units. Report your answer to the hundredths place and do not include units.