Q: 1. Why was it important to use "flat" soft drinks for your titrations? Would your calculations of…
A: Here we are titrating soft drink which contains acids with strong base, NaOH to find the citric acid…
Q: What is the solubility of Mg(OH)₂ at a pH of 11.20? (Ksp Mg(OH)₂ is 1.6 × 10⁻¹³)
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Q: A student weighs out 0.9854 g of Na2CO3 unknown and dissolves it in 25.00 mL of deionized water. A…
A: Answer % of Na2CO3 in the unknown = 54.05% Formulas No.of moles = Given…
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A: Given that: pH = 12 Ksp for Mg(OH)2 = 5.61×10-12 To find, molar solubility of Mg(OH)2?
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Q: Titrate 1.2035g of solid KHP (KC8H5O4) requires 23.89 mL of an unknown NaOH solution to reach the…
A: Given: Mass of KHP = 1.2035g Volume of unknown NaOH = 23.89mL= 0.02389 L To find: The molarity of…
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A: Given: MgO is being titrated using sulfuric acid. Normality of titrant i.e. H2SO4 = 1.017 N
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A: GIVEN:-
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Q: How many milliliters of 0.118 M HCl are needed to titra (a) 48.2 mt of 0.0708 M RbOH 19 72578 Xmt…
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Q: Question 2
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A: Answer: 35.5 mL
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Q: In an acid base titration lab, a student determined that a NaOH solution was 0.1885 M. The student…
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A: Given: Molarity of concentrated H2SO4 solution = 2.50 M Volume of diluted H2SO4 solution = 50 mL…
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A: The given problem can be solved by using Henderson-Hasselbalch equation given below as; pH=pKa + log…
Q: Titrate 1.2035g of solid KHP (KCeHsO4) requires 23.89 mL of an unknown NaOH solution to reach the…
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Q: 1. A student weighed out 0.300 grams of a monoprotic acid (HA) and added 50.0 mL of DI water to the…
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Q: Titrating a 25.00 mL aliquot of 0.150 M NaOH with 0.250 M HCl will require 0.94 mL 41.67 mL…
A: 15.00 mL
Q: Calculate the molarity of NaOH (40 g/mol) solution if 12.25 mL was used to titrate 0.2615 gram of…
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Q: (3)) To adjust a NaOH solution, 0.1128 g H2C2O4 2H20 is weighed and dissolved in 25.0 mL of…
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Q: A sodium hydroxide (NaOH) solution was standardized with KHP primary standard. The concentration was…
A: A neutralization reaction is one where an acid reacts with a base to form salt and water. The…
Q: A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach…
A: Given data, Volume of Ca(OH)2 solution = 50.0 mL Molarity of HNO3 = 0.340 M Volume of HNO3 at…
Q: An instrument used to measure the acidity or alkalinity of a solution.
A: As per bartleby guidelines I answered only first question so please don't mind.Thanks in advance.
Q: A solution of hydrazoic acid, HN3 (43.03 mg/mmol), a colorless, volatile, and explosive liquid, was…
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Q: a student mixes the following solutiond. what is the ph of the solution? .2 L of .1 M Ca(OH)2 .3…
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Q: 3..If a 0.2250g sample of 96.5% NaHCO3 is titrated with 0.1165N H2SO4, what volume of the acid was…
A: Given, A 0.2250g sample of 96.5% NaHCO3 is titrated with 0.1165N H2SO4, the volume of the acid was…
Q: 250 ml volume of a mixture of 0.8g of NaHCO3 and 0.2g of NaOH in water. Take 50 ml of this mixture…
A: Moles of NaHCO3 in 5o mL = mass of NaHCO3molar mass of NaHCO3 x 50250 = 0.884 x 15 = 0.0019 mol =…
Q: IDENTIFY IF THE GIVEN STATEMENTS ARE TRUE OR FALSE In the assay of sodium bicarbonate, three moles…
A: Since you have posted a question with multiple sub-parts, we will solve first three subparts for…
Q: 1,Titrate 15.00 mL of 0.256 M KHP solution requires 20.75 mL of an unknown NaOH solution to reach…
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Q: If a 325 mg sodium bicarbonate tablet is titrated with 5.11 mL of 0.9165N HCl, what is the % label…
A: Solution -
Q: Propanoic acid has a Ka=1.3x10-5. The titration starts with 40.00 mL of 0.1000 M propanoic acid…
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Q: A 0.5000 g sample contains NaHCO₃, Na₂CO₃ , and NaOH, either alone or in permissible combination.…
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A: Given, Ca(HCO3)2 = 4.86 ppm Mg(HCO3)2 = 7.3 ppmCaSO4 = 6.8 ppmMgSO4 = 9.0 ppmMgCl2…
Q: 4,Titrate 0.5687g of solid KHP (KC8H5O4) requires 13.52 mL of an unknown NaOH solution to reach the…
A:
Q: Titration of a 0.492-g KH₂PO4 used 25.6 mL of 0.112M NaOH. What is the percent purity of KH₂PO4? MW…
A: The number of moles of a substance is determined as the mass of the substance upon its molar mass.…
Q: 50 mL sample solution containing Na2CO3 and NaOH is titrated with 0.2 M HCl solution. Acid…
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Q: A 0.217 gram sample of a diprotic acid requires 14.1 mL of 0.100 M NaOH to titrate the acid to its…
A: Weight of sample= 0.2 17 g Volume of NaOH=14.1mL Concentration of NaOH=0.100M Molecular weight of…
Titration of a 0.824 g of 99.99% KHP (204.23 g/mol) with phenolphthalein required 18.3 mL of NaOH (40.00 g/mol) solution to reach the end point. The same titrant was used to analyze an impure acetic acid (CH3COOH, 60.06 g/mol) solution. A 10.0 mL aliquot of the sample required 12.9 mL of the titrant.
What substance served as the primary standard?
Which served as the indicator in the titration?
What is the color at the end point?
What is the concentration of the titrant?
What is the molar concentration of the acetic acid solution?
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- cedric and astrid titrated a 15.00 ml aliquot of grapefruit juice with a 0.134 M NaOH solution to the end point. the initial buret reading was 1.04 ml and the final buret reading was 24.83ml. H3C6H5O7(aq) + 3 NaOH(aq) yeilds Na3C6H5O7(aq) + 3 H2O)(l) The volume of NaOH titrated is 23.79ml 24.83ml - 01.04ml = 23.79ml of NaOH ***What is the mass of citric acid in the juice sample? 0.204g of H3C6H5O7 ( can you please show how to calculate this answer)Bay Water Titration The concentration of Cl- in ocean water is about 500-600 mM. The baywater is diluted by a factor of 12.5 using a 20.00 mL volumetric pipet and a 250 mL volumetric flask. Using a 15.00 mL volumetric pipet, 15.00 mL is transferred into three clean Erlenmeyer flasks. 10 mL of 1% dextrin solution, 20 mL of de-ionized water, and 3-4 drops of indicator are added and titrated each with the AgNO3 solution. From the procedure, find: Dilution factor Volume of diluted bay water Then calculate: The [Cl-] of diluted bay water The [Cl-] of bay water Consider this information: [AgNO3] = 0.04043177 trial # Veq 1 13.91 2 13.73 3 13.9 4 13.86 5 13.87 6 13.84 average 13.85167 [Cl-]Bay = ([AgNO3](Veq(ave))/Vdil bay water pipeted) (Vflask/Vbay water)Oxalic acid dihydrate (H2C2O4 2H2O) can be used to standardize NaOH solution through acid-base titration. To determine the molarity of an unknown NaOH solution, a student weighed out 0.56 g of solid oxalic acid dihydrate and dissolved the solid in 32.8 mL of DI water. The resulting solution was used in a titration with the unknown NaOH solution (3 drops of phenolphthalein was used as an indicator). The balance chemical equation is given below. If the student used 21.21 mL of the unknown NaOH solution in the titration, what is the molarity of the NaOH solution? Keep the correct number of significant figures. H2C2O4 (aq) + 2NaOH (aq) --> Na2C2O4 (aq) + 2H2O (l)
- Oxalic acid dihydrate (H2C2O4 2H2O) can be used to standardize NaOH solution through acid-base titration. To determine the molarity of an unknown NaOH solution, a student weighed out 0.56 g of solid oxalic acid dihydrate and dissolved the solid in 32.8 mL of DI water. The resulting solution was used in a titration with the unknown NaOH solution (3 drops of phenolphthalein was used as an indicator). The balanced chemical equation is given below. If the student used 25.71 mL of the unknown NaOH solution in the titration, what is the molarity of the NaOH solution? Keep the correct number of significant figures. H2C2O4 (aq) + 2NaOH (aq) --> Na2C2O4 (aq) + 2H2O (l)A pharmacist is identifying the saponification value of corn oil in the lab. She weighs 1.8 g of corn oil and saponified with 25 mL of 0.4 N KOH which require 9 mL of 0.5N HCl to titrate the excess KOH. She performs blank determination, 20 mL of 0.5 N HCl was required to titrate the corn oil. What is the saponification value of the corn oil? Does the sample comply with the USP requirement? Use this formula to work your result Saponification Value = (Vblank - Vsample)N of HCl56.11/Sample weight (g)Sulfamic acid ( +H 3NSO 3 - , 97.094 g/mol) is a primary standard that can be used to standardize NaOH. +H 3NSO 3 - + OH - → H 2NSO 3 - + H 2O What is the molarity of a sodium hydroxide solution if 34.26 mL reacts with 0.3337 g of sulfamic acid?
- IDENTIFY IF THE GIVEN STATEMENTS ARE TRUE OR FALSE In the assay of sodium bicarbonate, three moles of the titrant react to 2 moles of the analyte. One milliliter of 1N sulfuric acid is equivalent to 84.01 grams or 1 mEq of sodium bicarbonate. A weak acid when titrated with a weak alkali will give a sharp endpoint. When a weak acid is titrated with a strong alkali, methyl red is used as an indicator. To have a balanced equation in the assay of sodium bicarbonate, the titrant should have a coefficient of one and the sulfate salt of sodium produced should have a coefficient of three. The standard acid solutions used in acidimetry and alkalimetry are usually prepared from HCl or H2SO4. When a weak alkali is titrated with strong acid, the indicator used is methyl red.4 Sodium bicarbonate is considered as the primary standard in its own assay. When a strong alkali is titrated with a strong acid, phenolphthalein may…In the titration of 25.00 mL of a water sample, it took 19.040 mL of 4.965x 10−3 M EDTA solution to reach the endpoint. The total hardness is always listed in parts-per-million (ppm) of CaCO3 (or mg CaCO3 / Kg H2O). Since the density of water is 1.0 g/mL, one ppm would be the same as the number of mg of CaCO3 per liter of water. Determine the number of moles of CaCO3 present in the titrated sample of water, assuming that all the Ca2+ combines with CO32−. (enter your answer with 3 significant figures)A solution contains NaHCO3 (84.01 g/mol), Na2CO3 (105.99 g/mol), and NaOH (40.00 g/mol), either alone or in permissible combination. Titration of a 25.0-mL portion to a phenolphthalein end point requires 29.75 mL of 0.1205 M HCl. A second 25.0-mL aliquot requires 36.56 mL of the HCl when titrated to a bromocresol green end point. What is the general composition of the solution? Calculate the no. of mg of each solute per mL of solution.
- 1. Why was it important to use "flat" soft drinks for your titrations? Would your calculations of the molarity of citric acid have been too high or low if you hadn't used a "flat" soft drink? 2. Grape juice contains diprotic acid, tartaric acid, which has the molecular formula C4H6O6. If 20.00 mL of grape juice required 36.00 mL of 0.0500 M NaOH for the titration to a pink endpoint, what is the molarity of tartaric acid on the grape juice? 3. Diet Big Red soda contains citric acid, as shown in the ingredient list below, Carbonated Water, Citric Acid, Natural and Artificial Flavors, Sucralose, Sodium Benzoate, Caffeine, Malic Acid, Red 40, Acesulfame Potassium, Phosphoric Acid, and Acacia Gum What are two obvious reasons that we did not try to determine the citric acid content in a "flat" sample of Diet Big Red soda?A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach the endpoint, a total of 16.3 mL of HNO₃ was required. write the balanced chemical equation for the reaction. How many moles of HNO3 are used in the titration? How many moles of Ca(OH)2 had to be present in the initial reaction? What was the concentration of the initial Ca(OH)2 solution?Starting a titration, the technician requires 200mL of a 0.22% (w/v) solution of citric acid, anhydrous. The technician should weigh out 4.4g of this compound. (True or False) Could you explain how you got to the answer.
