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- Helppp nowwowoow please Equation #H+MA.VA=MB.VB #OH- What is the concentration of an unknown Mg(OH) 2 solution if it took an average of 15.4mL of 0.100M solution to neutralize 10.OmL of the Mg(OH) 2 solution ? What is the concentration of an unknown LiOH solution if it took an average of of 0.100M HNO3 solution to neutralize 20.0ml of the solution?HELPP NOWWWW Equation :#H +MAVA=MBVB #OH- Question 1) what is the concentration of a unknown Mg (OH)2 solution if it took an average of 15.4mL of .100M HCL solution to neutralize 10.0 mL of the Mg (OH)2 solution Question 2) what is the concentration of an unknown LiOH solution if it took an average of 25.4mL of .100 HNO3 solution to neutralize 20.0mL of the LiOH solutionAt 55°C aniline, CH NH₂, has a Kb = 8.2 *10-1⁰ What is the pH of a 0.035M solution in water? (Please type answer)
- What is the hydronium ion concentration (in mol/L) of an aqueous solution with a pH of 3.4? State your answer in scientific notation using three significant figures. Example: The value 1.23 × 10-6 has three sig. figs. You need to enter this value the following way: 1.23e-6 That means the part " × 10 " of the number is replaced by just "e" which stands for exponent.Draw a curve for a series of solutions of HF. Plot [H3O+]total on the vertical axis and the total concentration of HF (the sum of the concentrations of both the ionized and nonionized HF molecules) on the horizontal axis. Let the total concentration of HF vary from 11010M to 1102M.Part D Part complete Pancreatic juice, pH = 7.9 Pancreatic juice, = 7.9 acidic basic SubmitPrevious Answers Correct Part E Part complete Estimate [H3O+] value for pancreatic juice. Express your answer using one significant figure. [H3O+] [H3O+] = 1×10−8 M SubmitPrevious Answers Correct Significant Figures Feedback: Your answer 1.26⋅10−8 = 1.26×10−8 M was either rounded differently or used a different number of significant figures than required for this part. Part F Estimate [OH−] value for pancreatic juice. Express your answer using one significant figure. [OH−] [OH−] = nothing M
- What is the percent dissociation of 0.257 M weak acid (HA) with a Ka of 3.3x10-7 at 22.7°C? Please type answer note write by hend.NOTE: gas constant R=8.315 J/mole*K1.The pH of a sample Ais 11, while the pH of sample Bis pH 9. Sample A has:A)a hundred times more[H+] as sample B. B)a thousandtimes more[H+] than sample B. C)a hundred times less[H+] than sample B. D)a thousandtimes less[H+] than sample B. E)ten thousandtimes more[H+] than sample B.How many grams of NH4Cl (53.49 g/mol) must be dissolved in 4.670 L of solution in order to obtain a solution that has a pH equal to 5.46? The Kb of NH3 at the temperature in this problem is 5.2 × 10-5. The Kw can be assumed to equal 1.0 x 10-14. Report your answer to the tenths place and do not include units. Tip: What is the reactant? Start by writing the reaction with water that is taking place and the corresponding Keq expression. You do not need an ICE table.
- Determine the initial concentrations of the species below, after the solutions are mixed. Volume0.0350 MKMnO4(mL) Volume0.0650 MH2C2O4(mL) VolumeH2O(mL) InitialConcentrationKMnO4(M) InitialConcentrationH2C2O4(M) (3 significant figures) (3 significant figures) 1.00 1.00 18.00 2.00 2.00 16.00 3.00 3.00 14.00 4.00 4.00 12.00 5.00 5.00 10.00Baseline Question: Calculate the pH of a 5.6x10-9M HCl aqueous solution. ANS: pH=6.99 Commentary: Since I know HCl is a strong acid and ionization is 100%, I thought I could find pH as -log(5.6x10-9), however my teacher said that was incorrect . She did a Kw=[OH-][H3O+] to find x. Use image below to see my work. The answer to the question is pH= 6.99. Actual Question:I want to know why we had to do an ICE table and find "x" (another H3O concentration) instead of -log(5.6x10-9).What is the percent ionization of a 0.35 M HCN solution (Ka = 5.8 x 10-10)? Answer in 2 Sf.