A 0.1-L unbuffered solution needs the pH adjusted from 3.5 to 2. How many microliters of a 12 molar HCI solution need to be added to adjust the pH? Report your answer to four decimal places.

Determine the pH of a solution that is prepared by dissolving 7.2 g of Ba(OH)2 in 4.7 L water at 25°C. Assume that the volume of the solvent does not change upon addition of the solute. Atomic Weights: Ba = 137.3 g/mol; O = 16.00 g/mol; H = 1.008 g/mol. Express your answer in two decimal places only. Do not put the units.

A Calculate the pH of an aqueous solution that contains 6.5 x 10 M Ca(CH)z at 25 °C. Provide your answer in two decimal places: this is the number of significant figures in the given value. (Hint: Consider the number of OH" units that will dissociate once Ca(O); dissolves in water.) Your answer. SUBMIT YOUR SOLUTION ON THE NEXT PAGE. B. Using two acids, HF and CH,CO,H, and their conjugate bases, write a Bronsted Lowry acid base reaction that has an equilibrium constant greater than one. pka of HF: 3.2 pka of CH,CO,H 4, 75 SUDMIT YOUR ANSWER ON THE NDXT PAGE.

You have a 48.5 g mixture that contains potassium propanoate (CH3CH2COOK) and Propanoic acid (CH3CH2COOH). This mixture is placed in a flask and made up to reach 2 L. after a period of time determines that the pH of this solution is 5.8. Calculate the composition of the mixture. Ki =1.34x10-5

Please don't provide handwritten solution ....

Consider the following information to answer the questions below. A volume of 10.00 mL of 0.100 M acetic acid (HC2H3O2) is titrated with 0.107 M sodium hydroxide solution. Given the chemical equation below. Calculate the volume (in milliliters) of NaOH needed to reach the equivalence point of the titration. HC2H3O2(aq) + NaOH(aq) -> H2O (l) + NaC2H3O2(aq)

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.

Consider the following chemical equilibrium: HCOO¯¯ (aq) + H₂O(aq) = HCOOH(aq) + OH¯(aq). Which of the following graphs represents the perturbation on the system and the change of pH when HCI is added to the container? | pH time || III pH ↑ time Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. C Q a || = III = d IV pH IV pH time time K Open Χ Your answer

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=

Calculate the amount of 6M HCl required to neutralize the solutions in beakers #1 and #2. Note: Saturated NaHCO3 has a concentration of about 1.1M. (use the last page for your calculations)