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- A solution has a pOH of 4.5. What is the concentration of H3O+ in the solution in Molarity? Group of answer choices 0.0000316 M 0.00000316 M 0.00316M 3.16 x 10^-10 M 3.16 x 10^-11 M 3.16 x 10^-13 Marrow_forwardHelppp 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?arrow_forwardDetermine 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 10.00arrow_forward
- 4. Calculate the moles of H2O that can be obtained from 15.0 mL of 0.250 M HClaccording to the following equation:2 KMnO4(aq) + 16 HCl(aq) → 2 MnCl2(aq) + 5 Cl2 + 8 H2O(l) + 2 KCl(aq)arrow_forwardDetermine the pHpH of an HNO2HNO2 solution of each of the following concentrations. Part A 0.510 MM Express your answer to two decimal places. pHpH = nothing SubmitRequest Answer Part B 0.110 MM Express your answer to two decimal places. pHpH = nothing SubmitRequest Answer Part C 1.40×10−2 MM Express your answer to two decimal places. pHpH = nothing SubmitRequest Answer Part D In which cases can you not make the simplifying assumption that x is small? In which cases can you not make the simplifying assumption that x is small? only in (b) only in (a) in (b) and (c) in (a) and (b) SubmitRequest Answer Provide Feedback Nextarrow_forwardTITRATION First: 10 mL - unknown acid + 0.15 Phenolphthalein solution = 10.150 mL Next: 10.150 mL + 0.77 mL of 10.0 M NaOH = 10.92 mL unknown acid @ 25.0 degrees celsius What is the concentration (M) of the acid (Please use 3 significant figures) = ???arrow_forward
- Chemistry 4. Solution D: 20.0 mL of 1:1 buffer + 5.00 mL NaOH. [NaOH] = 0.1108M [HCl] = 0.1153M pKa(acetic acid) = 4.68 pH = 5.19 Calculate the stoichiometric concentrations of HAc and Ac- in soulution D, after mixing the buffer and base. Show all of your work, including your ICE table and calculations. Clearly list the data used in your calculations.arrow_forwardA mixture of 20.0ml of 0.10M Ba(NO3)2 with 50.0ml of 0.10M Na2CO3. what is the cation concentration in the final solution?arrow_forwardA HNO3 solution has a sp.gr. of 1.42 and is 70.0 % (w/w) HNO3 . How many ml of this solution is needed to prepare 250. mL of 1.00 M HNO3?arrow_forward
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