Consider a flask containing 50.00 ml. of 0.0426 M trimethylamine ((CH,),NH,). This is titrated with a 0.0957 M hydrochloric acid solution from a burette. Given: K, of (CH,), NH, is 6.5 x 10-5, 1.1 Determine the pH of the solution in the flask after 28.00 mlL of the acid has been added? You must show any reaction equation(s) that you may think are necessary. 1.2 Determine the pH of the solution in the flask at the half-way point of the titration.
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- .6. A certain weak base has a ?b of 8.50×10−7. What concentration of this base will produce a pH of 10.28? 7. For the diprotic weak acid H2A, ?a1=2.0×10−6 and ?a2=5.1×10−9. What is the pH of a 0.0400 M solution of H2A? What are the equilibrium concentrations of H2A and A2− in this solution? Answer bothDetermine the pH of the following solutions, given that Ka (HF) = 6.8 x 10-4.Hint: 1. Diagnose the scenario (i.e. strong acid + weak base, etc.), 2. If buffer solution, make useof Henderson-Hasselback eqn and 3. If strong acid/base added to buffer, write out reaction withstrong acid or base on the left hand side, then calculate ICE change. a. 0.5 moles of NaF b. A solution with 0.5 moles HF (Ka = 6.8 x 10^-4) and 0.5 moles NaF, to which 0.1 moles HClis added."M" in .25M represents what? Question 4 options: Concentration None of the above Color pH
- ITTL/ What is the pH of 92.9 mL of a solution which is 0.29 M in NaCN and 0.61 M in HCN? For HCN use K₂ = 4.9x10-10. Your Answer:Consider a solution initially containing 0.30 M of CH3NH2 mixed with 0.50 M of CH3NH3Cl in water. What is the pH after the addition of 6.415 mL of 0.10 M NaOH to 19.41 mL of this solution? (Kb for CH3NH2 = 4.47 × 10–4) Express your answer using at least three significant figures. Do not use scientific notation.PLease this time I need explanation. The last time was just solved and I didn't know how the volumes were found in mL. 1. Calculate the pH when 40.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹) 2. Calculate the pH when 29.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)
- Hello I am gettin 2 answers for the same question, which one is correct. The question is as follows. If we have a 25 mL solution of weak acid HA (Ka = 1,00 * 10-6) and at pH 4,00. How much water needs to be added to change the pH to 5.5? Here is a link to the first answer, wich is about 19 L and the second answer that is less than a Liter. It is a lot of diffrence in the answers, I am more confused now than I was before using bartleby!!! Can I really trust the rest of your answers? first https://www.bartleby.com/questions-and-answers/if-we-have-a-25-ml-solution-of-weak-acid-ha-ka-100-10-6-and-at-ph-400.-how-much-water-needs-to-be-ad/b9a38e6b-a610-4117-935d-f1eeb5a632ee second https://www.bartleby.com/questions-and-answers/if-we-have-a-25-ml-solution-of-weak-acid-ha-ka-100-10-6-and-at-ph-400.-how-much-water-needs-to-be-ad/09629357-da08-413b-8c84-c62b6dddf337Calculate the theoretical pH of this buffer solution(25mL of 1.0 M HC2H3O2 and 25mL of 1.0 M NaC2H3O2). The actual pH of the buffer was 4.44, now compare it to the theoretical value you calculated Info given pH 4.44 Ka= 1.8X10-5What is the pH of a solution of a freshwater solution at 25C containing 3mM DIC = H2CO3 + HCO3- + CO3^2? ( Please type answer note write by hend )
- Question 11 Calculate the pH of mixing 90 mL of 0.19 mol/L hydrazine (H2NNH2) with 80 mL of a 0.14 mol/L H2NNH3Br solution. After determining the pH, again determine the pH of this same solution if 6.50 mL of 0.300 mol/L HNO3 is added.Give both answers to at least 3 decimal places.In Trial 1 0.5 grams of KHP were dissolved in 100 mL of water and titrated with 18.56 mL of NaOH that was later determined to be 0.132 M. Calculate the [C8H4O42-]EqPt , [OH-]EqPt, kb, pOH and pH values for the solution at the Equivalence Point.Question: Determine the Molar Concentration of Diazepam, if its pH=8.56, and has a pKa of 3.0 May I get a detailed solution for this question I seem can't to get the correct solution pattern? The answer to this question I believe is 1.3183M