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What is the pH of a buffer that is 1.5 M in H2CO3 and 1.0 M in NaHCO3? Show your work.
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- A 1.50 g sample of lithium nitrite, LiNO2, is added to 100.0 mL of water. Acid dissociation constant for HNO2, Ka = 5.6 x10-4 M. a) Determine whether the resulting solution is acidic or basic. (Be sure to show your work) b) Calculate the pH of the resulting solution.Part A You are asked to prepare a pH =3.00 buffer solution starting from 1.40 L of a 1.00 M solution of hydrofluoric acid (HF) and an excess of sodium fluoride (NaF). What is the pH of the hydrofluoric acid solution prior to adding sodium fluoride? Express your answer to three significant figures. VO ΜΕ ΑΣΦ pH= 0 Submit Previous Answers Request AnswerWhat is the pH of 0.150M of Na2HPO4? How to determine 1st or 2nd intermediate? ka1 7.11*10-3 ka2 6.34*10-8 ka3 4.22*10-13
- Select all of the solutions from the first part of the experiment that you would expect to be acidic (i.e., have a pH less than 7.0). 0.5 M NaNO2 1 M NaHCO3 2 M H₂SO4 0.5 M Na2SO3 rainwater (water equilibrated with CO₂) 2 M NH4OHThe Ksp for In(OH)3 is 1.3 x 10-37. Find the pH of an In(OH)3 saturated solution. Find the concentration of In3+ in a buffered solution at pH 5 Find the concentration of In3+ in a buffered solution at pH 6 Find the concentration of In3+ in a buffered solution at pH 7 Please answer complete question this all parts of a questionConsider a buffer solution prepared by adding 0.45 mol of CH3COOK to 1.00 L of 2.00 M CH3COOH. (K₁ = 1.8 x 10-5). If 0.05 mol of HCI is added to this buffer solution the pH of the solution will drop slightly. The pH does not drastically decrease because the HCI reacts with present in the buffer solution. Select one: O a. H₂O O b. CH3COOH O C. CH3COO O d. H+
- 2. When 30 .00 mL of 0.1011 M HCl in 50 mL of deionized water is titrated against 0.09889 M NaOH, the pH increases. What is the volume (in mL) of NaOH required to reach the equivalence point and a pH of 7.00? Find the pH when the volume of NaOH added is 0.02 mL less than the volume required to reach the equivalence point. Find the pH when the volume of NaOH added is 0.01 mL less than the volume required to reach the equivalence point. Find the pH when the volume of NaOH added is 0.02 mL more than the volume required to reach the equivalence point. Comment on the significance of the changes in pH values in relation to the increments of sodium hydroxide added when going “through” the end point. Define equivalence point. For a weak base/strong acid titration, is the pH at the equivalence point <, >, or equal to 7?6. a. Calculate the pH of a buffered solution that is 0.100 M in C6H5CO2H (benzoic acid, Ka = 6.4 x 10-5) and 0.100 M NaC6H5CO2. b. Calculate the pH after 20.0% (by moles) of the benzoic acid is converted to benzoate anion by addition of a strong base. Use the dissociation equilibrium: C6H5CO2H (aq) + H2O (l) ⇌ C6H5CO2- (aq) + H3O+(aq) c. Do the same as in part b, but use the following equilibrium to calculate the pH: C6H5CO2 -(aq) + H2O(l) ⇌C6H5CO2H (aq) + OH- (aq) d. Do your answers in part b and c agree? Explain.What is the pH of a solution that is 0.0100 M HCN and 0.0200 M in NaCN? Ka (HCN) = 6.2 × 10-10.. Calculate the pH of a solution of 0.10 M acetic acid. Calculate the pH after 50.0 mL of this solution is treated with 25.0 mL of 0.10 M NaOH. Ka (CH³COOH) = 1.8 × 10-5.
- You have three known solutions: 1) Na,co, 2) Ваcl 3 ) ΚNO, Even though you know that you have these three solutions, you do not know which one is which because they are not labeled. Which one of the following reagents should you add to each solution to be able to accurately identify and label them? Select one: A. Cacl, X B. We need more than one of these reagents to be able to identify all three solutions С. NaOH D. HCI E. H,SO,Weak base: 25 mL of 0.00255 M hydroxylamine HONH2 (Kb = 1.1 × 10-8) Strong acid: 0.001545 M HNO3. Questions 1-2 were previously explained and answered. Can you explain numbers 3, 4, and 5. Answers are on the side to check if your work matches answer. Conditions to determine: 1. Initial pH – Answer: 8.7 2. pH at 10.12 mL of titrant added – Answer: 6.5 3. pH at equivalence point – Answer: 4.5 4. pH 1 mL of titrant added after the equivalence point– Answer: 4.4 5. pH 15 mL of titrant added after the equivalence point– Answer: 3.53. A formic acid buffer is prepared with 0.010 M each of formic acid (HCOOH) and sodium formate (NaCOOH). The Ka for formic acid is 1.8 x 104. What is the pH of the solution? What is the pH if 0.0020 M of solid sodium hydroxide (NaOH) is added to a liter of buffer? What would be the pH of the sodium hydroxide solution without the buffer? What would the pH have been after adding sodium hydroxide if the buffer concentrations had been 0.10 M instead of 0.010 M? eit af