7. A sample of 10.0 mL of concentrated sulfuric acid, H,SO, is used to make 475 mL of a 2.5 M sulfuric acid solution. What was the initial concentration of the sulfuric acid?
Q: What volume (in L) of 3.50 mol/L sulphuric acid solution is needed to make 100.0 mL of 0.450 mol/L…
A: Given, For Concentrated sulfuric acid solution: Concentration of sulphuric acid solution (M1) = 3.50…
Q: How many grams of iron(II) acetate are in 19.89 g of a 2.49 % by mass iron(III) acetate solution?
A: Given data : Mass of iron acetate = 19.89 g Mass percent =2.49% Formula used : Mass percent =…
Q: What mass of NaCl is present in 125.0 mL of a 0.100 M NaCl solution?
A: Volume of solution in L = 125/1000 = 0.125 L Since molarity = moles of solute / volume of solution…
Q: A solution is prepared by mixing 20.0 mL of methanol with enough water to produce 400. mL of a…
A: Given - - > Volume of methanol mixed = 20.0 mL Volume of the solution formed = 400.0mL Percent by…
Q: What volume of a 5.0 M CaCl2 solution do you need to make 1.0 L of a 0.1 M CaCl2 solution?
A: Since you have asked multiple questions, we will solve the first question for you. If you want any…
Q: 5. A stock solution of potassium nitrate, KNO, has a concentration of 1.5 M. What volume of dilute…
A: Dilution of the solution: On dilution of the solution with the pure water, the mole of solute…
Q: a. For a solution of 0.206 mol of potassium dichromate in 0.500 L. What is the molarity and mass of…
A: Since you have asked multiple question, we will solve the first question for you. If you want any…
Q: ow many g of barium fluoride are needed to prepare 43.6 mL of a 1.55 M solution of barium fluorid
A: The molarity is the concentration term which is the number of moles of solute per liter volume of…
Q: How many moles of CaCl2 are present in 10.0 mL of 0.600 M CaCl2 solution?
A: Given: Volume =10mL=0.01 L Molarity of solution=0.600M Moarity=no of moles of solutevolume of…
Q: 715 mL of water was added to 40.0 mL of 0.550M MgCl4 solution. Assuming the volumes are additive,…
A: Dilution of the solution: When we dilute a concentrated solution with pure water, the mole of solute…
Q: Silver nitrate solutions are often used to plate silver onto other metals. What is the maximum…
A: Mass percentage is an important method to find out the concentration of a solution. It is expressed…
Q: water should be added
A:
Q: Commercially available concentrated hydrochloric acid is 12.4 M HCl. Calculate the volume of…
A: Given that, the concentration of HCl is 12.4 M. We have to prepare 2.00 L of 1.50 M HCl solution.…
Q: KCl is 1.61% by mass in 54.6 g of water. Calculate the mass of KCl present in the solution
A:
Q: The volume of 13.7 M H2SO4 solution required to prepare 285 mL of 1.17 M H2SO4 is _________mL.
A: Here we have to calculate volume of H2SO4 needed to prepare 285 mL, 1.17M H2SO4 solution-
Q: 1 How many grams of KBr are needed to make 350 mL of a 0.500 M solution? A. 4.50 g B. 56.4 g C 20.8g…
A: “Since you have asked multiple question, we will solve the first question for you. If you want any…
Q: Copper(II) sulfate solution is used to etch designs on copper jewellery. Calculate the volume in L…
A:
Q: What is the molarity of an aqueous solution prepared by adding 36.4g of barium chloride (208.23…
A:
Q: A 8.0 m NaCl solution would have what mass percent of NaC in the solution? The molar mass of NaCl is…
A: Molality is the way to express the concentration of any solution. It can be defined as the number of…
Q: What is the molarity of an aqueous solution prepared by adding 36.5g of barium chloride (208.23…
A: Number of moles of barium chloride in solution = given mass / molar mass = 36.5 g / 208.23 g/mol =…
Q: Calculate the volume of 0.250 M solution made by dissolving 5.56 g of solid magnesium chloride in…
A: Given Molarity of solution ( M ) = 0.250 mole/Liter Mass of MgCl2 = 5.56 gram Volume = ? Molar…
Q: If 67.1 g of CaCl2 is added to 275 g of water, calculate the mass percent of CaCl2 in the solution
A: Given, mass of CaCl2 = 67.1 g Mass of water = 275 g Mass % is calculated as a mass of a component…
Q: 4. Calculate the percent by volume of a solution created by adding 75.0 mL of acetic acid to 725 mL…
A: Percent by volume is equal to the volume of acetic acid divided by the volume of solution multiplied…
Q: a) Determine the mass of ammonium nitrate dissolved in 750 mL of a 3.82 mol/L solution.…
A: Given: Initial volume V1= 750mL= 0.75L Final volume V2= 5.0L Molarity M1 = 3.82M
Q: 1. Determine the mass (in grams) of sodium chloride needed to prepare a 500.0 mL of a 2.0 M…
A: Given data: Volume of solution = 500.0 mL Molarity of solution = 2.0 M
Q: Chemistry labs often purchase concentrated HCl (12.0 M) and dilute the solution for laboratory use.…
A: Molarity of initial solution = 12.0 M Molarity of new solution = 0.250 M Volume of new solution =…
Q: How many grams of sulfuric acid H2SO4 are needed to make 250 ml of a 1.22 M solution
A: Given :- molarity of solution = 1.22 M or 1.22 mol/L Volume of solution = 250 ml or 0.250 L To…
Q: If you dilute 175 mL of a 1.6 M solution of LiCl to 1.00 L, determine the new concentration of the…
A: Concentration of a solution is the amount of solute molecules dissolved per Liter of solution. It is…
Q: 6 M of HCl solution is required for the chemical analysis. How much water must be added to 250 mL…
A: Given: Initial concentration (stock solution), M1 = 12 M The initial volume (stock solution), V1…
Q: A solution of nitric acid has a density of 1.400 g/mL and is 13.250 M. Calculate the percent HNO3 by…
A:
Q: 7. The concentration of stomach acid, HCl, is approximately 0.10 M. What volume of stomach acid…
A: Given; Note: 1g = 1000 mg , 1L = 1000 ml
Q: To 14.8 cm3 of a 1.5 M H2SO4 , enough water is added to produce a 0,18 M H2SO4 solution. How much…
A: During the process of dilution, the number of moles of the solute H2SO4 remains the same. Thus, we…
Q: How would you prepare 580 mL of 8.3 M NaCl solution? Dissolve _______________g of NaCl in a minimum…
A: Given: Molarity of NaCl solution that has to be prepared = 8.3 M. Volume of the NaCl solution that…
Q: A diluted NaCl solution is made by mixing 110.5 mL of 1.26 M NaCl with 201.3 mL of water. What is…
A:
Q: solution
A:
Q: Commercially available concentrated sulfuric acid is 18.0 M H2SO4. Calculate the volume (in mL) of…
A: Dilution is a process via which the concentration of a solution is decreased by adding extra…
Q: 1. What is the molar Concentration of a 500 mL solution containing 0.3 mol of glucose? A. 0.15 mol/…
A: The number of moles of glucose is = 0.3 mol The volume of the solution is = 500 mL The molar…
Q: What mass (in grams) is necessary to create a solution of 0.570 m HCl with 250.0 g of water? The…
A: Given,M = 0.570 m HClV= 250.0 g of water.The molar mass of HCl is 36.46 g/mol.
Q: solution is prepared by mixing 8.37 g of sodium carbonate with 154. mL of water. What is the…
A:
Q: What is the concentration of a solution made by diluting 65 mL65 mL of 6.0 M HCl6.0 M HCl to a final…
A: Given information: Volume of HCl (V1) = 65 mL Concentration of HCl (C1) = 6.0 M New volume of HCl…
Q: What is the molarity of the solution formed by mixing 2 mol of sodium hydroxide with enough water to…
A: Given: Moles of sodium hydroxide= 2 mol The volume of solution = 1.14 L Molarity is defined as…
Q: What volume of 2.0 M NaCl solution can be made from .75 moles of NaCl?
A: Here, we have to find the volume of 2.0 M NaCl solution that can be made from 0.75 moles of NaCl.
Q: What volume of 3.25 mol/al stock solution is needed to make 2.5L of 1.50 mol/L solution?
A: Given: Stock solution concentration = 3.25 mol/L. Final solution concentration = 1.50 mol/L. And…
Q: How many moles of sodium hydroxide, NaOH, are present in 1.58 L of a 0.160 M sodium hydroxide…
A: Since molarity = moles of solute / Volume of solution in L Volume of solution in L = 1.58 L and…
Q: Hydrochloric acid is usually purchased in a concentrated form that is 37.0% HCl by mass and has a…
A:
Q: 1. A 0.10 M HNO3 solution will be prepared from concentrated HNO3. a. Using the method outlined in…
A: Given, density =1.42 g/ml 70% by mass HNO3 is given Molarity =? Molar mass of HNO3 = 63g/mol
Q: 175 mL of a 3.6 M aqueous solution of LiCl is diluted with water to a final volume of 2.0 L. What is…
A: Given, M1 = 3.6 M V1 = 175 ml = 0.175 L V2 = 2.0 L M2 = ?
Q: 1. A 0.10 M HNO3 solution will be prepared from concentrated HNO3. Using the method outlined in…
A:
Q: A 225 mL sample of a 10.0 M aqueous stock solution is diluted to 4.00 L upon addition of water. What…
A:
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- Shortly after the dissolution of lead(IV) oxide, the dissolvedPb4+ will react with water to form dissolved speciesand according to the following stoichiometric equation andchemical equilibrium coefficients. This will continue pullingPbO2(s) into solution, causing higher overall leadconcentrationsIt is required to know the concentration of an aqueous solution of H2SO4 that appeared in the laboratoryChemistry III and it's unlabeled. To this end, a student of analytical chemistry carried out the followingProcedure: He took 5.00 mL of a fresh and standardized solution of 0.525M NaOH and brought them to a250.0 mL balloon to be completed with distilled water. Subsequently, he poured 15.00 mL of the solutionH2SO4 of unknown concentration in an Erlenmeyer flask and added 2 drops of phenolphthalein.Using a burette filled with the last NaOH solution, he noticed that when adding 39.40 mL of the hydroxidethe Erlenmeyer solution reached a faint but permanent pink. With the above dataDetermine the concentration and pH of the H2SO4 solution.A. This is the equilibrium constant for the reactionin which a solid salt dissolves to give its constituent ions in Chemicalequilibrium constant Solubilityproduct constant Idealgas constant Noneof these B. Directprecipitimetry: Van’tHoff Method VolhardMethod MohrMethod Gay-LussacMethod C. Molecules which provide a group ofattachments used in Maskingagents Demaskingagents Ligands Chelatingagents D. Substances that determine the concentrationof a metal in the presence of another metal Maskingagents Demaskingagents Ligands Chelatingagents E. EDTAis an example of a: Masking agent Demaskingagent Ligand Chelatingagent For numbersF to H, identify the component of the chemical reaction: PO4-3 + H3O+ → HPO4-2 + H2O. Select from the following choices: Acid Base Conjugateacid Conjugatebase F. PO4-3 G. HPO4-2 H. H2O For numbers I to L, consider the given chemical equation: NH3(aq) + H2O(l) ↔ NH4+(aq) + OH-(aq) I Thechemical reaction from the given…
- In gravimetric analysis, volatile electrolyte is used in peptization step a. to form small nucleib. to easily dry precipitatec. to reprecipitate the analyteexplain pleaseWhat is meant by non-stoichiometric defect? Ionic solids which have anionicvacancies due to metal excess defect develop colour. Explain with the helpof suitable example.Sudies have revealed extremely high deposits of heavy metals and paryiculate matterin rivers , making them unwholesome for drinking. With your on analytical separation and analyses, outline a suitable analytical separation protocol that can be employed to recover polluted river bodies and make wholesome for drinking. Explain in details.
- https://www.youtube.com/watch?v=eX3JiKmenuU Describe the color change observed when the heated crystals were dissolved in water.Calculate the molar concentration of FeSCN2+ in solution #3. The determined molar absorptivity of the solution at 448 nm is 333 L mol-1 cm-1.While working in a metal processing facility, Letlen had accidentally mixed two metal vatstogether creating an alloy. One vat was labeled for cadmium, while the other was not. It canbe assumed that these are of pure metal composition. To identify this metal, Letlen took 1.000 g of the homogenous alloy sample composed ofcadmium and the unknown metal, dissolved, and diluted it to exactly 100.0 mL in avolumetric flask. A 20.00-mL aliquot was taken and titrated this using 22.82 mL of 0.05000M EDTA. In a second 20.00-mL aliquot, the Cd was masked through the addition of HCN/NaCN buffer.The titration of the unknown metal in the aliquot required 15.13 mL of EDTA.MW: Cd (112.411 g/mol) a. Calculate the moles of Cd and the moles of unknown metal in the 20.00-mL aliquot.b. Calculate the moles of Cd and the moles of unknown metal in the sample.
- IFs undergoes autodissociation into IF4 and IF6. SbFs acts as an acid and KF acts as a base when dissolved in IFs. Write balanced chemical equations for these reactions.What mass of solid Lanthanum (III) oxalate nonahydrate { La2 ( C2O4 )3 ∙ 9 H2O } can be obtained from 650 mL of 0.0170 M aqueous solution of LaCl3 by adding a stoichiometric amount of sodium oxalate ? with solution/explanationi) Silver ion (Ag+) reacts with SCN- ion to form silver thiocyanate (AgSCN). What change will the student observe when a solution containing Ag+ ion is added to the mixture? ii) Briefly explain how your answer to is consistent with Le Chatelier’s principle.