What is the pH at the equivalence point in the titration of a 23.4 mL sample of a 0.477 M aqueous nitrous acid solution with a 0.362 M aqueous barium hydroxide solution? pH =
Q: A 40.0 mL volume of 1.80 Fe(NO3)3 is mixed with 21.5 mL of 0.808 M Fe(NO3)3 solution. Calculate the…
A: Given, A 40.0 mL volume of 1.80 Fe(NO3)3 is mixed with 21.5 mL of 0.808 M Fe(NO3)3 solution, i.e.…
Q: titrated 18.00 mL of HCl solution with 58.6 mL of 0.145 M NaOH solution to the endpoint. (See…
A: Using , M1V 1=M2V2
Q: A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs…
A: It is acid-base titration. We knew that sodium hydroxide is not the primary standard solution. So we…
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Q: Consider a 0.238 M aqueous solution of sodium hydroxide, NaOH. How many grams of NaOH are dissolved…
A: Since, Number of moles = Concentration × Volume
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A:
Q: A sample of solid Ca(OH)2 was stirred in water at a certain temperature until the solution contained…
A: Given, Volume of calcium hydroxide = 87.5mL Molarity of HBr = 0.0892 M Volume of HBr = 68.7 mL
Q: magnesium sulfate
A: To find the final concentration of of pb+2 remaining in solution
Q: 17. What is the concentration of NaCl in a solution if titration of 15.00mL of the solution with…
A: Volume of NaCl = 15.00 mL Concentration of AgNO3 = 0.2503 M Volume of AgNO3 = 20.22 mL
Q: An Erlenmeyer flask contains 41.40 mL of a hydrochloric acid. The solution is titrated and reaches…
A: Here we are required to find the concentration of HCl solution .
Q: 19- A sample of limestone is titrated for its value as a neutralizing agent. A sample weighing 1.000…
A: Limestone is CaCO3 Moles of CaCO3 = 1 / 100 = 0.01
Q: 2. Suppose a titration needed 27.15 mL of 0.2497M HCI solution to completely react 25.00mL Ba(OH)2…
A: The number of moles of a substance is determined as the mass of a substance upon its molar mass. The…
Q: The lead in a 0.2000-g sample is precipitated as PbCrO4. The precipitate is filtered, washed, and…
A: The balanced equations are Pb2+ + 2 CrO42– --------> PbCrO4 (s) 2 PbCrO4 + 2 H+ -------> 2…
Q: Complete the double displacement reactions and balance the reaction. Indicate if the reaction does…
A: Inorganic chemistry.
Q: The equivalence point for the titration of a 25.00-mL sample of CsOH solution with 0.1062 M HNO3 is…
A: Given,
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Q: concentration
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Q: A permanganate solution is standardized by titrating it with a 0.1712 M SO,2- solution. The balanced…
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Q: You titrated a 21.00 mL solution of 0.0500 M oxalic acid with a freshly prepared solution of KMnO4.…
A: Given, Volume of oxalic acid = 21.00mL. Molarity of oxalic acid = 0.0500M. Volume of KMnO4 solution…
Q: A certain solution of KMnO4 is being prepared to treat water and has a concentration of 14.50%…
A: Given: The solution of KMnO4 = 14.50 %(m/V).........(1).
Q: A 25.00 mL sample of acetic acid (CH3COOH) is titrated to the equivalence using 31.08 mL of 0.1978 M…
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Q: A 0.5504-g sample of KHP (potassium hydrogen phthalate, KHC8H4O4; molar mass = 204.22 g/mol) is…
A:
Q: A 30.00 ml sample of phosphoric acid is titrated with a 0.050 M magneisim hydroxide solution. The…
A: Given: Volume of sample = 30.00 mLInitial buret reading = 4.71 mLFinal buret reading = 31.09…
Q: A 4.500-g sample containing sodium carbonate (105.99 g/mol) and other impurities is titrated with…
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Q: 10.00-mL sample of dilute sulfuric acid, H2SO4, is titrated with 0.2540 M NaOH solution and 35.20 mL…
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Q: 7.7.3 Zinc sulfate eye drops Zinc sulfate solution has been traditionally used as an astringent and…
A: In this case, the quality of Zn2+ ions in the eye drops is being checked. By quality, we mean we…
Q: What volume of a 0.462 M NaOH solution would be required to titrate 2.85 g of pure KHP
A: In acid base titration, all H+ neutralised by OH- . Here from mass of KHP we can determine moles of…
Q: 1. a: A sample of 8.5 mL H,SO, is titrated with 18.5 mL of 0.35 M Ca(OH),. What is the concentration…
A: Answer : Molarity and volume of solution con be calculated as follows
Q: 1-A 0.2954-g sample of an unknown monoprotic acid is dissolved in water and titrated with…
A: Given, Monoprotic acid: HX Potassium hydroxide: KOH mass of sample of an unknown monoprotic acid =…
Q: Na2CO3, can be titrated with HCl according to the following balanced chemical equation.…
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Q: The end point in a titration (stoichiometric / equivalence point) of a 50.0 mL sample of aqueous HCl…
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Q: Titration of 0.2121 g of pure Na2C2O4 (134.00 g/mol) required 43.31 mL of KMnO4. What is the molar…
A: From the given reaction, it is clear that 2 mol of MnO4- reacts with 5 moles of C2O42-to form the…
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Q: The following solutions are needed to be prepared for the titration procedure: 1. 20 mL of 2 M HCl…
A: The titration process wherein 1.0867 grams of Fe(OH)n was mixed with the 20 mL of 2 M HCl that you…
Q: In a common medical laboratory determination of the concentration of free chloride ion in blood…
A: Given: Concentration of Hg(NO3)2 = 8.35×10-4 M Volume of Hg(NO3)2 = 1.64 mL Volume of Cl- = 0.25 mL…
Q: The titration below was performed by placing 10.00 mL solution in an Erlenmeyer flask and titrating…
A: The given volume of the basic solution present in the Erlenmeyer flask (V1) = 10.00 ml Molarity of…
Q: KHP (potassium hydrogen phthalate, KHC8H4O4
A: Molarity = Moles of solute/ volume of solution (in L) Moles = Mass in gm/molar mass
Q: A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs…
A: Number of Mole- Ratio of given mass of substance to the molar mass of substance is called number of…
Q: 18. In a common medical laboratory determination of the concentration of free chloride ion in blood…
A: Given that: Molarity of Hg(NO3)2 = 0.000825M Volume = 1.46ml = 1.46ml×1L/1000ml = 0.00146L Molarity…
Q: A 19.95−mL sample of HCl of unknown concentration was transferred to a flask, a few drops of the…
A: The neutralization reaction of HCl and NaOH is given as:HCl (aq) + NaOH (aq) → NaCl (aq) + H2O…
Q: A solution of Ba(OH)2 is titrated into a solution of HOI. Calculate the volume of 0.140 M Ba(OH)2…
A: Interpretation - To determine the volume 0.140 M Ba(OH)2 (aq) needed to reach the equivalence point…
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Q: A 20.00 ml sample of a Ba(OH)2 solution is titrated with 0.245 M HCI. If 27.15 mL of HCI is…
A: Since you have asked a multiple question, we will solve the first question for you. If you want any…
Q: A 15.00 mL solution of phosphoric acid (H;PO4) is titrated with 11.20 mL of 0.155 M sodium…
A:
Q: Potassium permanganate, KMNO4, is both effective at treating water and has medicinal uses. A certain…
A: Given: Concentration of KMnO4 in %(m/v) = 17.49 % Assuming 1 L i.e. 1000 mL of the solution.
Q: A 4.500-g sample containing sodium carbonate (105.99 g/mol) and other impurities is titrated with…
A:
Q: Instead of using ratios for back titrations we can also use molarities, if our solutions are…
A: Step 1: First of all, the moles of Al(OH)3 is obtained from the given data. But, here the data is…
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- What is the pH at the equivalence point in the titration of a 23.0 mL sample of a 0.357 M aqueous acetic acid solution with a 0.341 M aqueous barium hydroxide solution? (Ka=1.8 x 10 -5) Please post clear explanation or dont respond thanks so much...A RbOH solution is titrated four (4) times against potassium hydrogen phthalate (KHP; FW=204.224) samples to the Phenolphthalein endpoint. Using the data below, determine the concentration of the RbOH solution? g of KHP Volume of Base Required 0.5373 g 42.49 mL 0.5856 g 43.88 mL 0.5790 g 48.56 mL 0.5856 g 44.60 mL (Report your answer as "mean +/- std dev") M What is the percent relative standard deviation? % What is the 99% Confidence Interval for the concentration of the solution (population mean)?Molarity of titrant (NaOH): 0.4550 M HC2H3O2 (aq) + NaOH (aq) → NaC2H3O2 (aq) + H2O (l) Trial # First Second Third Fourth Initial buret reading 0.15 mL 2.43 mL 1.32 mL 0.58 mL Final buret reading 18.62 mL 20.87 mL 20.03 mL 19.14 mL Volume of titrant used 18.47 mL 18.44 mL 18.71 mL 18.56 mL 4) Calculate the molarity of the acetic acid in the vinegar solution (Show your work). use FW for moles-->grams acetic acid. Molarity acetic acid = _____________ M 5) Calculate the weight % of acetic acid in the vinegar. How does this compare with the % listed on the label (5.00%)? (For this calculation assume that density of vinegar is 1.03 g/mL and of course, show your work). Weight % = ___________ 6) If you didn’t get the same weight % of acetic acid as listed on the vinegar label (5.00 %), what are two things (be specific) that could’ve happened during the experiment that could explain the variation from the expected weight %? To do…
- Calculate the molarity of a dilute Ba(OH)2 solution if addition of 58.22 mL of the base to 0.602 g of benzoic acid (MW=122.12g/mole) required a 5.4129 mL back-titration with 0.01248 M HClA sodium hydroxide (NaOH) solution was standardized with KHP primary standard. The concentration was found to be 0.1022 M. What is the concentration of a 25.0-ml hydrochloric acid (HCl) solution if it required 32.6 ml of NaOH to reach the phenolphthalein end point?A 50.00 ml solution of 0.0400 M (Kb=5.6x10-4) is titrated with 10.00 mL of a 0.200M solution of hydrochloric acid as the titrant. What is the pH at the equivalence point? (Kw=1.0x10-14)Choose the option. a. 2.63 b. none of the above c. 6.38 d. 3.25 e 6.11 f 7.62
- 10- A solution with a volume of 100 ml is prepared by weighing 2.50 g from the mixture of Kl and KBr. When 10 ml of this solution is titrated with 0.015 M AgNO3 solution, there is a consumption of 105. Accordingly, calculate the percentage of Kl in the mixture A)88,4 B)43,7 C)56,3 D)11,6Determine the molarity of the 10.00 mL standard EDTA solution titrated using 1.000 g zinc sulfate in 100 mL solution. (ZnSO4 = 161.47 g/mol ) 0.006193 M 0.6193 M 6.193 M 0.06193 MA 25.0mL mixture solution contains NaNO3 and KIO4, titrated against 0.02M Na2S2O3. The volume of titrants is 18.2 mL, the concentration of KIO4 is:a) 3.64 × 10-4 b) 9.1 × 10-5c) 1.82 × 10-3 d) 2.35e) 3.64 × 10-4
- A saturated solution of the hypotheticl salt MA2 has a M+ ion concentration of 0.000669 M. What is the value of Ksp with 3 significant figures. MA → M2+ + 2 A-You want to measure the concentration of carbonate (CO32-) in a mildly basic solution by using an EDTA back titration. CaCO3 has a Ksp of 5x10-9. You add 50.00 mL of 0.3484 M CaCl2 to 500.0ml of sample and filter the solution to remove the precipitate. You then take 250.0 mL of the filtered solution and titrate with 0.1786 M EDTA. You require 23.72 mL to reach the endpoint. What is the concentration of carbonate in the original sample?A 75.0-mLmL volume of 0.200 MM NH3NH3 (Kb=1.8×10−5Kb=1.8×10−5) is titrated with 0.500 MM HNO3HNO3. Calculate the pHpH after the addition of 28.0 mLmL of HNO3HNO3.