Which of the ff statement is TRUE when 60 mL of 0.02000 M Mno, has been added to 50.00 mL of 0.05000 M U Select one: O The amount of u and Mno, reagent are equal. O The Mno, reagent is in excess. O This is the equivalence point. O The U reagent is in excess.
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- Consider the reaction shown below. (a) How many milliliters of 0.1550 M KMnO4 are needed to react with 132.0 mL of 0.1550 M oxalic acid? mL(b) How many milliliters of 0.1550 M oxalic acid are required to react with 132.0 mL of 0.1550 M KMnO4? mLcalculate weight of AgCl when added excess of AgNOs to 0.75g of BaCl2 if M.wt AgCl=143.3 and M.wt BaCk=208.3 AgNO3+ BaClz + BaNOsI add 0.1011 g of a primary standard FAS into a volumetric flask and diluted it to the line with water. We then add 2 mL of that solution into another 100 mL volumetric flask and diluted to the line with water. What would be the concentration of the diluted solution in g/mL?
- Quantity Your Data 1. Grams of vinegar sample used for your titration 25.000 g 2. Initial Buret Reading of Sodium Hydroxide solution 10.00 mL 3. Final Buret Reading of Sodium Hydroxide solution 28.00 mL 4. Amount of Sodium Hydroxide Solution used to neutralize the vinegar sample 5. Concentration of NaOH in the NaOH solution 0.050 g/mL 6. Grams of NaOH used to neutralize the vinegar 7. Grams of acetic neutralized by the amount of NaOH 8. Percent acetic acid in the vinegar Hints: For #4, The amount of NaOH used is the difference between the starting buret value and the ending buret value. For #6, Once you calculate the amount of sodium hydroxide used, multiple that value by the concentration of NaOH in the NaOH solution. For #7, Multiply the value obtained in number 6 by the number 1.5. Remember, we learned that every 1 gram of NaOH neutralizes 1.5 grams of acetic acid. For #8, Divide the grams of acetic acid by the grams of vinegar sample and multiply this value by…What is the pHpH after the addition of 10.0 mLmL of 0.140 MNaOHMNaOH to 25.0 mLmL of 0.110 MHNO3Prepare 100.00 mL of a solution with the following chemicals; solid FeCl3 6H2O, iron(II) chloride hexahydrate (source of FeCl3) dilute hydrochloric acid in the rack – 3.0 M solid sodium salicylate – 99.7% assay Concentrations: FeCl3: 0.020 M HCl: 0.050 M Salicylate (mg/L): 40.25 PLEASE SHOW HOW TO CALUATE AND WORK. The only equations you will need to use are the equations for molarity and dilutions.
- In this experiment, you will determine the amount (percent) of potassium hydrogen phthalate (KHP) that is in an impure sample. You will determine the percent of KHP via titration using NaOH with known molarity. The reaction will follow, KHC8H4O4 (aq) + NaOH (aq) ---------> KNaC8H4O4 (aq) + H2O (l) At the endpoint, the moles of KHP will equal the moles of NaOH. You will use phenolphthalein as the indicator. The endpoint of the reaction will be a light pink solution color. How will you know the reaction is over? About how much KHP will be used in the titration? Which 3 substances go into the 250 mL Erlenmeyer flask for the titration? What is the mole to mole ratio in the reaction of KHP and NaOH? What solution goes into the buret?10. A 21.70 mL volume of 0.0940 M NaOH is required to reach the phenolphthalein endpoint in the titration ofa 3.06 g sample of vinegar. a.Calculate the number of moles of acetic acid in the vinegar sample. b.Calculate the mass of acetic acid in the vinegar sample. The molar mass of acetic acid is 60.05 g/mol. c.Calculate the percent by mass of acetic acid in the vinegar sample. Assume the density of the vinegar is 1.00 g/mL. Express the percent acetic acid in the vinegar to the correct number of significant figures.A 25.00 mL sample of a vinegar solution is diluted to 250.00 mL with water. Then a 25.00 mL aliquot of the diluted sample is titrated with strong base, requiring 22.13 mL of 0.1027 M sodium hydroxide to reach the endpoint. What is the molar concentration of acetic acid in the original sample of vinegar before the dilution?(a) 2.278×10‒3 M(b) 2.278×10‒2 M(c) 0.09091 M(d) 0.9091 M
- 3. how would the following errors affect the concentration of Cl- obtained in question 2b? give your reasoning in each case. a. the student read the molarity of AgNo3 as 0.02104M instead of 0.02014M b. the student was past the endpoint of titration when he took the final buret reading.6. Some sulfuric acid is spilledon a lab bench. You can neutralizethe acid by sprinkling sodiumbicarbonate on it and then moppingup the resultant solution. The sodiumbicarbonate reacts with sulfuric acidas follows:2 NaHCO3(s) + H2SO4(aq)Na2SO4(aq) + 2H2O(l) + 2CO2(g)Sodium bicarbonate is added until thefizzing due to the formation of CO2(g)stops. If 27 mL of 6.0 M H2SO4 wasspilled, what is the minimum mass ofNaHCO3 that must be added to thespill to neutralize the acid?I need to figure out how to calculate the molar mass of this unknown acid by titration , and give some errors why the ideal molar mass was not obtained? Mass of acid used: 2.4060 grams Buret initial volume : 0.00mL End volume of buret: 99.4 mL [NaOH]=0.1501M unknown #122 : molar mass 152.15 g.mol for error analysis