2. If a water sample contains 10 mg/L of bicarbonate alkalinity and pH=8, what is the carbonate alkalinity in mg/L as the ion, in mg/L as CaCO,, and in meq/L. pKal=6.35 and pKa2=10.33. pKa=-log10 (Ka) and there are two Ka (K1 and K2) as shown below. [#* [#CO;] H' K, = [#*[co?]. K, THCO;"]

Q: What is the pH of an aqueous solution that is 0.1M NH4Cl? The Kb value for NH3 is 1.8 x 10-5

A:

Q: pH. Vol (mL). Midpoint 1. 2.99 Midpoint 1= w-2.99 Midpoint 2= w-6.56 Mass of unknown sample =.122g.…

A: Answer: In the given acid-base titration, weak acid is being titrated against strong base where weak…

Q: If 300 ml of 0.30 M phosphate buffer at pH 6.8 is added to 200 ml of 0.075 M NaOH, what is the…

A: A buffer is a solution which shows resistance to show change in pH when acid or base is added to it…

Q: Consider the titration of 40.0 mL of 0.11 M H3A (Kal = 8.4 x 10-4, Ka₂ M KOH. = c. At 60.0 mL of KOH…

A: Answer: of weak tricprotic acid is titrated with 0.11 M KOH. The values for the given triprotic…

Q: A volume of 500.0 ml. of 0.110 M NaOH is added to 585 mL of 0.250 M weak acid (K,= 8.02 x 10-5).…

A:

Q: 34. The presence of CO32", HCO3 and CO2 in body fluids helps to stabilize the pH of these fluids…

A: Given: The value of Ka,1 is 4.2×10-7. The value of Ka,2  is 4.7×10-11. Introduction: Buffer refers…

Q: How many grams of KHCOO (MM = 84.12 g/mol) must be added to 1.00 L of 0.256 M HCOOH to make a buffer…

A: pH of an acidic buffer solution can be calculated from Henderson hasselbalch equation. pH = pKa +…

Q: Consider a buffer solution that contains 0.30 M H3PO4 and 0.10 M NaH2PO4. pKą(H3PO4)=2.16. X…

A: Given : solution contain 0.30 M H3PO4 and 0.10 M NaH2PO4 pKa of H3PO4 = 2.16 Calculation of 1. 2.…

Q: 4) How many grams of potassium azide (KN3, MM = 81.118 g/mol) are present in 250.0 mL of a pH 4.20…

A: Buffer is a solution which has a specific pH and resist a change in its pH when any acid or a base…

Q: Which of the following substances is best for preparing a buffer solution with pH=9 and a buffer…

A: pH = 9Buffer ratio = [base]/[Acid] = 1

Q: How many grams of potassium napthenate (KC11H7O2; MW=210.27 g/mole; Kb=85x10-10) must be added to…

A:

Q: b. Calculate the change in pH when 25 mL of 1.0 M HCl is added to the buffer solution.

A:

Q: Determine the mass of solid NaCH:COO that must be dissolved in an existing 500.0 mL solution of…

A: Given that : Concentration of acetic acid = 0.200 M Ka = 1.8 x 10-5

Q: A buffer solution is made that is 0.495 M in H₂CO3 and 0.495 M in KHCO3. Kat for H₂CO3 is 4.20 x…

A: Answer: Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: Vitamic C, aka ascorbic acid (H₂C₆H₆O₆) is a weak diprotic acid. Which of the following aqueous…

A:

Q: Consider a buffer solution made up of H2PO4- and HPO42- . For H2PO4-, Ka = 6.2 x 10-8. What mole…

A: Answer: 1.38

Q: Q3|| A. Calculate the PH of the (0. 1 N) Na;PO, in 250 ml B. What is the Normality of a sulfuric…

A: The given data contains, concentration of Na3PO4=0.1 N

Q: calculate the pH of the equivalence point N2OH soluhon Concentrahun.of n =0.lmol/L Mean titre (MOOH…

A: A titration is  an analytical method that is used to determine the unknown quantity of the analyte…

Q: Calculate the pH of a NH4* buffer syster 0.010 M NH4CI.

A: Basic buffer pOH , Henderson equation is pOH = pKb + log (nsalt / nbase)  Where  pKb o NH3 = 4.74…

Q: A 15.00 ml aliquot of a 0.75 M solution of a weak acid (Ka = 1.50E-04 at 25°C) is titrated with…

A:

Q: A- Explain the pH variations when a 25 ml of 0.IM HCI solution that titrated with (0, 12, E.P., 25.5…

A: Q2.A. The above example is strong acid vs Strong base titration. H+ + OH- ---> H2O Amount of HCl…

Q: A buffer solution is made that is 0.495 M in HNO₂ and 0.495 M in NaNO2. (1) If K, for HNO₂ is…

A: Given,  Molarity of HNO2 = 0.495 M Molarity of NaNO2 = 0.495 M Ka of HNO2 = 4.50 × 10-4 moles of KOH…

Q: 0 / 6 ptsWhich of the following buffer systems is best for a buffer with [OH–] equal to 1.00 × 10–7…

A: The objective of the question is to identify the best buffer system for a solution with a hydroxide…

Q: A student wants to complete neutralize a 5.00g sample of K₂CO3 with a stock solution of 0.15M H3PO4.…

A: Given:Mass of K2CO3 = 5.00 gConcentration of H3PO4 = 0.15 MBalance this equation:A balanced chemical…

Q: Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC4H,O2 with 0.100 M Sr(OH)2…

A:

Q: As a technician in a large pharmaceutical research firm, you need to produce 450. mL of 1.00 mol L…

A:

Q: What is the pH of a 1.0 L solution that is 0.50 M PO43- and 0.50 M HPO42-? (The pKa values for…

A: As per the Henderson–Hasselbalch equation:pH = pKa + log [PO4-3]/[HPO4-2]pKa = 12.4 as ( third…

Q: Which of the following would be the best choice to prepare a buffer with pH = 3.00 ? A. C5H5N:…

A: Acidic buffer solution - a buffer solution that made of weak acid and its conjugate base ( strong…

Q: What is the pH of a solution made by adding 23.5 g of KC2H302 to 400 mL of 0.80 M HC2H302? (Ka for…

A:

Q: Choose the representative solubility equilibrium at pH 9.0 using the following data. Cu 2+ 8.0 Cu…

A: Given:A maximum amount of a substance( solid) that is dissolved in a given amount of solvent at a…

Precipitation Titration

Precipitation analysis is used to analyze drugs, and to measure the salt content in food and beverages. It is an important concept from the examination point of view many practical questions are asked on the topic. This topic is significant in the professional exams for both undergraduate and graduate courses, especially for