A patient weighs 164 pounds (1.000 pound = 0.454 kg). The patient requires a dose of a drug that is 4.50 mg/kg of body weight. You have a stock solution of the drug that is at a concentration of 60,000 ppm. The density of the stock solution is 1.16 g/mL. The drug has a molecular mass of 623.87 g/mol. You decide to give the patient the drug using an i.v. bag (intravenious injection) with a volume of 1.00 L and pump it into the patient at a rate of 10.0 ml/min. What volume of the stock solution of the drug do you need to add to the i.v. bag in order to ensure that the patient gets the correct dose?

Calculate the volume of stock glucose solutions (2.5 % and 15%) that need to be used to prepare 800 mL of glucose solution with a concentration of 13%. In this case % refers to the grams of glucose per 100 mL of water. V1= volume of stock solution with concentration C (2.5%) V2= volume of stock solution with concentration C2 (15 %) You need to determine V, and V2 in mL

1a. Medical saline typically consists of 4.50 g of NaCl in 500.0 mL of solution. What is the molarity of this solution? What is the molality of this solution? (Use the density of water = 1 g/mL; for this question, since the concentration is dilute you may assume that the added NaCl does not result in a change in volume when it is added to water.) Do your answers make sense? Would either of these values potentially depend on temperature? 1b. Stomach acid is essentially a solution of hydrochloric acid (HCl). When first secreted, stomach acid has a concentration of roughly 0.160 M HCl. How many moles of HCl are present in 50.0 mL of stomach acid? 1c. If 5.0 mL of saline is introduced to 15 mL of stomach acid. What is the mole fraction of NaCl? What is the mole fraction of HCl? (In your calculations, use the molarities from parts (a) and (b) above).

Diuril is a prescription drug used to treat hypertension. You are given a 2.5 g vial of Diuril, with negligible volume, and asked to prepare a solution by combining with 20.0 mL of sterile water. What is the final concentration in mg/mL?

A stock solution whose concentration is 25.00 mg/mL was provided. A primary standard solution was then prepared by transferring 5.00 mL of the stock solution into a 50.00 mL volumetric flask. The primary standard solution was used to prepare three standard solutions of different concentrations by taking different volumes of aliquots into three 25.00 mL volumetric flasks: Standard Solution #1 #2 #3 Amount of Primary Solution (mL) 5.00 10.00 15.00 Three 25.00 mL volumetric flasks were then diluted to mark with water. Questions #1 What is the concentration of the primary standard solutions, expressed in units of mg/ml? #2 Re-write the concentration of the primary standard solutions obtained from Q#1 in units of μg/mL. #3 Determine the concentrations of three standard solutions in units of µg/mL. #4 What is a requirement for a "blank" solution used in calibration in spectrophotometry? Page 5 (Experiment #3)

The blood serum acetone for a person  is determined to be 23.7 mg of acetone per 100 mL of serum. Express this concentration %v/v if the density for acetone liquid is 0.79 mg/mL.

H2S + 2 NaOH  Na2S + 2 H2OCalculate the normality of a solution that contains 3.10 grams of H2S in 843 mL of solution.  ____N

Then, why  8.56 % = (42.8 g/volume of the solution) × 100 % Volume of the solution = [(42.8 × 100)/8.56] mL becomes 500mL not 500g?

A patient is given an IV drip at a rate of 110 mL per hour for a total of 6.2 hours. The IV has a calcium ion concentration of 5.94 mEq/L. How many grams of calcium ion were delivered to the patient through the IV?

A student wants to make a 250 mL stock solution with a concentration of 1000 mg -P/L. The student has an unlimited amount of KH2PO4 and DI water. What mass of KH2PO4 is needed to make 250 mL the 1000 mg -P/L solution?  Using the stock solution from the previous question, what volume of stock is needed to make a 20 L solution with a concentration of 0.1 mg -P/L?