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[DOC File]Molar Mass - jdenuno
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molarity of dilute and undiluted vinegar M1V1 = M2V2 Dilute: M1 = 0.1 M NaOH V1 = volume NaOH from a, above M2 = _____ V2 = 1.0 mL Undiluted: (Hint: the concentration of the dilute vinegar is 0.10 x that of the original vinegar sample!) molar mass of acetic acid (Hint: the formula for acetic acid is CH3COOH)
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[DOC File]Concentration Review Worksheet
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To solve problem 1, you need to have calculated for various parts that there are 2.08 moles of NaOH (which has a molar mass of 40 g/mol), that there are 750 grams of water (which has a density of 1 g/mL), and that there are 41.67 moles of water (which has a molar mass of 18 g/mol).
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[DOC File]MOLARITY / CONCENTRATION
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Calculate the mass of compound required to prepare 100.00 mL of a 1.40x10-2M CuSO4. Show your work. If 2.50g of NaOH are dissolved in 100.00 mL of water, what is the molarity of the solution? Show your work. If 10.00mL of the solution in question 2 are diluted to 100.00 mL, what will be the molarity of the dilute solution? Show your work.
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[DOC File]AP Chemistry – Chapter 3, Stoichiometric Relationships ...
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molar mass = 1.570 g/ 0.00611 mol = 257 g / mol . One point earned for determination of molarity One point earned for conversion of molarity to molar mass . OR, moles solute = ( T x kg solvent) / Kf = 0.00611 mol (one point) molar mass = 1.570 g / 0.00611 mol = 257 g / mol (one point) OR,
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[DOC File]Molarity Notes – H
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Example 1: Molar mass of salt (NaCl) is 58.5 g/mol, so if you dissolve 58.5g of salt in enough water to make 1.00 liter of solution, you have one mole of solute dissolved per liter of solution. The concentration of this solution is one molar (1.00 mol/L or 1.00M)
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[DOC File]Molar Mass - jdenuno
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Molar Mass KHP: Mass KHP/Molarity KHP (or B / C) Percent Error: A = 204.2 g/mol, and O is your calculated value from step D. Discussion: Summarize what you did and describe your results making specific reference to your data. All your statements must be supported by evidence from the lab.
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[DOC File]AP Chemistry study guide for Solutions (Chapter 11)
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molar mass = 1.570 g/ 0.00611 mol = 257 g / mol . One point earned for determination of molarity One point earned for conversion of molarity to molar mass . OR, moles solute = ( T x kg solvent) / Kf = 0.00611 mol (one point) molar mass = 1.570 g / 0.00611 mol = 257 g / mol (one point) OR,
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Molarity - Quia
Molarity, M. Molarity is a means of representing a solution’s concentration. In other words, it expresses how much dissolved solute can be expected from a given volume of solution. The . molar concentration or molarity, M, of a solution is used to indicate the number of moles of solute per liter of solution:
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[DOC File]Molarity Lab
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Since they know the volume they started out with they can compute the molarity using the calculated mass. Mr. Green was the murderer. I had great results with this lab, even if their lab techniques weren't perfect since the given range for Mr. Green was 0.5 - 1.5M anyway.
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[DOC File]MOLAR MASS
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MOLAR MASS. 1.) What is the molar mass of. a.) Na. b.) H2. c.) NH4. d.) C3H6Cl2. MOLARITY. 2.) What is the molarity of. a.) 3.62 mol NaCl in a 400.0 mL solution. b.) 0.36 g Na3PO4 12H2O in a 200.0 mL solution. c.) HCl if 130.0 mL water is added to 20.0 mL of a 0.5 M HCl solution . STOICHIOMETRY. 3.) What mass of Al(OH)3 is needed to create 6.0 ...
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Molar mass to molarity