Dry chemicals Sometimes you will need to make a solution of a specific molarity (M) from dry chemicals that need to be weighed. Recall that M units g/mole. You can use the equation below to determine the mass of the chemical you need to make the solution. = moles / L and the molecular weight of a chemical is in the Mass (g) = Molarity (M) * Volume (L) * Molecular Weight (g/mole) To get the units to cancel out, you need to use the units in the equation above. You can obtain t molecular weights from the bottle in which the chemical is stored (or by using a periodic table Example: Make 300 mL of 100 mM glycine 100 mM =0.1 M= 0.1 moles/L 300 mL = 0.3 L The molecular weight of glycine 75.07 g/ mol. %3D 0.1 moles/L 0.3 L 75.07 g/mole = 2.25 g of glycine %3D How much of the dry chemical is needed to make the following solutions? Your solvent will always be deionized water (DI H2O). Show your work. a. Make 25 mL of a 0.05 M glycine solution. The molecular weight of glycine is 75.07 g / r Make 500 mL of a 10 mM NaCl solution.

Dry chemicals Sometimes you will need to make a solution of a specific molarity (M) from dry chemicals that need to be weighed. Recall that M units g/mole. You can use the equation below to determine the mass of the chemical you need to make the solution. = moles / L and the molecular weight of a chemical is in the Mass (g) = Molarity (M) * Volume (L) * Molecular Weight (g/mole) To get the units to cancel out, you need to use the units in the equation above. You can obtain t molecular weights from the bottle in which the chemical is stored (or by using a periodic table Example: Make 300 mL of 100 mM glycine 100 mM =0.1 M= 0.1 moles/L 300 mL = 0.3 L The molecular weight of glycine 75.07 g/ mol. %3D 0.1 moles/L 0.3 L 75.07 g/mole = 2.25 g of glycine %3D How much of the dry chemical is needed to make the following solutions? Your solvent will always be deionized water (DI H2O). Show your work. a. Make 25 mL of a 0.05 M glycine solution. The molecular weight of glycine is 75.07 g / r Make 500 mL of a 10 mM NaCl solution.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A particular solution of hydrochloric acid is 3.0 M. How many moles of hydrochloric acid are present in 22.7 mL of this solution?
Will the calculated Molarity of NaOH be too high or too low or unaffected if the following happen: When you answer the question, consider how the situation affects the calculation of molarity of NaOH and moles NaOH, which is calculated from the mass of KHP. For each answer, you must supply a clear explanation for your answer. Often times, students will restate the facts rather than explaining why they chose the answer they chose. a) You add the weighed KHP to a flask containing a 60mL of water rather than 50 mL of water. Explain. Your answer must contain a well-thought-out and clearly written explanation. b) The buret is still wet with water on the inside when you add your NaOH solution. Explain c) The KHP is wet when you weigh it. Explain. d) You titrate past the equivalence point by 0.50mL Answer a-d
An aqueous solution is to be prepared that will be 3.87% by mass ammonium nitrate. What mass of NH4NO3 and what mass of water will be needed to prepare 1.23 kg of the solution? Mass = g NH4NO3 Mass = g water
5. You will also make other concentrations of solutions. If the concentration is to be less than a mole, reduce the mass of the substance accordingly. If the concentration is to be greater than 1M, increase BIOL 1406 the mass added or reduce the volume of water accordingly. Use this formula: Molarity = moles/liter. Example: Make a .5M solution of HCI Name: H = 1.008 Daltons CI = 35.45 Daltons Total = 36.46 Daltons = 36.46 grams .5M = X moles/1 liter .5M * 1 liter = X moles Date Number of moles = .5 .5 * 36.46 = 18.23 grams Add 500 mLs water to 1L volumetric flask, add the 18.23 grams HCI to the water, swirl to dissolve, then add water until it reaches the 1L or 1,000 mL mark. Answer the following questions: 1. How many mL should I use to make a 1M solution of MgBr2? ¶ 2. What is the mass of a mole of NH3? 3. How much CaCO3 should I use to make a 2M solution? 4. How much CaCO3 should I use to make a .25M solution? 5. What are the steps to make a 1M solution of NH3 - give the steps and…
4.67 g of cobalt(II) sulfate are dissolved in water to make 2600. mL of solution. Calculate the molarity. Isa molar mass needed for this calculation? Enter either yes or no, If so, calculate the molar mass using our periodic table and enter with the proper s.f. If not, enter 0. Do not include units. g/mol In the three blanks, enter the results of the calculation: value (decimal notation with proper s.f.)., units, and substance (in this order).
What is an aqueous solution? What is the difference between the solute and the solvent?
250. mL of water is added to 150. mL of a 2.32 M aqueous solution of glucose. The solution is then heated such that 50.0 mL of water is evaporated. What is the concentration of glucose in the final solution in units of M?
Suppose you are working with a NaOH stock solution but you need a solution with a lower concentration for your experiment. Calculate the volume (in mL) of the 1.100 M stock NaOH solution needed to prepare 250.0 mL of 0.1230 M dilute NaOH solution.
A www-awu.aleks.com/alekscgl FLJ-thPxaPpSwe. O O CHEMICAL REACTIONS Calculating molarity using solute mass 0/3 Dan A chemist prepares a solution of sodium nitrate (NaNO,) by measuring out 120. g of sodium nitrate into a 450. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's sodium nitrate solution. Round your answer to 3 significant digits. mol/L Explanațion Check 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use I Privacy Center Accessib solubility chem h.pdf 24 CH.9 PP ASSESS MacBook Air
1.) What mass of NaCl (in g) is necessary for 5.25 L of a 1.25 M solution? 2.) You have measured out 75.00 g of MgCl2 (formula weight: 58.33 g/mol) to make a solution. What must your final volume be (in L) if you want a solution made from this mass of MgCl2 to have concentration of 0.175 M? 3.) You have a concentrated solution of 5.00 M NaOH. If you dilute 365.2 mL of this solution with water to a final volume of 2.00 L, what is the molarity of the diluted solution? 4.) What volume (in mL) of 5.00 M HCl must diluted to a final volume of 1.50 L to make a solution with a final concentration of 0.470 M?
A chemist wants to make 3.0 L of a 0.558 mol L-1 CaCl2 solution. What mass of CaCl2 (in g) should the chemist use?
A chemist needs 225 mL of 2.3 M HCl. What volume of 12 M HCl must be dissolved in water to form this solution? (Ignore significant figures for this problem.)