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- The experimental pH of a 0.25 M solution of potassium hydrogen phosphate, K2HPO4, is 10.25. a. Is the solution acidic, basic, or neutral? B. Write the balanced net ionic equilibrium reaction. Identify the acid, base, conjugate acid, and conjugate base. Write the cquilibrium expression Kb for the reaction. C. Look up the theoretical pKafrom the CRC Handbook. Please give me all questions solution fastThe pH of a 0.0200 M solution of an unknown acid is 2.56. What is the Ka of this acid? To solve this problem: Write the acid dissociation equilibrium for the generic acid “HA” Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, A- and HA at equilibrium, in terms of x. What is x? Can you find it from the given information? You should be able to use the pH to get the concentration of H3O+, which is x. Do this. Now that you know x, plug in into the Ka expression and find Ka.Which acid would you choose to combine with its sodium salt to make a solution buffered at pH 4.25? For the best choice, calculate the ratio of the conjugate base to the acid required to attain the desired pH.chlorous acid (HClO2) pKa = 1.95 formic acid (HCHO2) pKa = 3.74nitrous acid (HNO2) pKa = 3.34 hypochlorous acid (HClO) pKa = 7.54
- Phenol Red: What is the purpose of this test? Why is a Durham tube inverted inside the test tube? At what pH does phenol red register an acidic result? What is the color? What is the color of an alkaline result? If you see an acid result, what does this mean? What about an alkaline result?Acidified potassium bromate(V), KBrO3, reacts with hydrogen sulfide, H2S, to give a yellow solid and an orange solution. On shaking the solution with trichloroethane, the trichloroethane layer turned orange-red. (a) Suggest the identity of yellow solid and the orange solution. Describe the type of reaction taking place. (b) Construct a balanced equation for the reaction between KBrO3 and H2S. (C) BrO3- is the conjugate base of HBrO3. Draw the dot and cross structure of HBrO3. (d) HBr is a stronger acid than HCl. However, HBrO3 is a weaker acid than HCIO3. Explain the difference in acidities.What is the predominant form of ammonia in a solution at pH 7.0? Approximately what fraction is in this form?
- How to answer for Ka/ Kb and calculated pH of a solution?I think solution 1,2 only has one Ka/Kb value then the other Sol. 3,4. Then with calculated pH, pH = -log[H+] (acid) and pH = 14 + log[OH-] (base) is utilized. Though I do not know how getting the Ka/Kb will be used to get pH Given: In a 10.0 mL 0.10 M CH3COOH solution, a 15 mL 1.00 M HCl solution was added. Compute for it's ka/kb and pH.Check the pH of aqueous solutions of primary, secondary and tertiary bromides in water by using 2 mL distilled water and 2 drops of the appropriate bromide. Are any of these solutions not neutral? If yes, write an equation to explain it. Would you expect the reaction to be SN1 or SN2?We can observe the common-ion effect in action by comparing how much a pure sample of acid dissociates to how much a sample of an acid dissociates when its conjugate base is in solution. Let's consider the oxoacid HIO, which has a Ka of 2.3×10-11. part 1: Calculate the pH of an aqueous solution of 0.100 M HIO. (Due to the low Ka value, you may apply the 5% approximation to avoid the quadratic equation if you wish.) part 2: Complete the RICE table for the dissociation of 0.100 M HIO in a solution with 0.0150 M IO- by selecting the correct answer from any dropdown boxes available. (Remember that the conjugate bases are typically added in as a soluble salt, such as NaIO, but that the salt dissociates completely and the alkali metal cation is a spectator ion.) part 3: Calculate the pH for the solution made from 0.100 M HIO and 0.0150 M IO- . For this case, you can also make the assumption that x will be negligibly small compared to the starting concentrations of the weak acid and…
- Q1.0 When 0.39 mol of solid CO2 is reacted with 0.23 mol of CH3MgBr in an ether solvent, the resulting product is isolated in aqueous solution (assuming 100% yield) and any excess CO2 is removed. Following this, 0.13 mol of HCl (aq) is added. What is the resulting solution's pH? Please note that you will need to research a pKa value for this query, and your answer should be reported to two decimal points.Calculate the pH of the solution after the addition of each of the given amounts of 0.0542 M HNO3 to a 60.0 mL solution of 0.0750 M aziridine. The p?a of aziridinium is 8.04. What is the pH of the solution after the addition of 0.00 mL HNO3? What is the pH of the solution after the addition of 6.20 mL HNO3?6.20 mL HNO3? What is the pH of the solution after the addition of a volume of HNO3HNO3 equal to half the equivalence point volume?A solution is prepared by combining 20.0 mLs of 0.10 M solution of an unknown acid and 15.0 mLs of 0.20 M conjugate base. The measured pH of this solution is 8.43. Use this information to calculate the pKa of the acid