You are working in an aseptic unit making TPN bags. One of your adult patients requires 20mmol of sodium ions added their bag.  You have a stock solution of 5% sodium chloride.  Relative molecular mass Na = 23.0, Relative molecular mass Cl = 35.5 How many mls of this stock solution are required?  Give your answer to one decimal place units – ml

A chemist must dilute 62.6mL of 2.81M aqueous sodium thiosulfate Na2S2O3 solution until the concentration falls to 2.00M. He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in milliliters. Be sure your answer has the correct number of significant digits.

3. A solution of 20.91 % by weight H,So, has a specific gravity of 1.150. What is the normality of this solution? Water is added to dilute this solution to a solution of 3.03% by weight H,SO, (SG= 1.020). What is the new normality of the resulting solution and how were they mixed? (Assume 100 ml of the original solution was used.)

What is the normality of a solution made by dissolving 10.00 g of hydrogen phosphate, H3PO4 in water to a volume of 150 mL? Note: Please present complete solution. Express your final answers up to two (2) decimal places.

To prepare olives for consumption and remove their bitterness, powdered soda (sodium hydroxide, NaOH) is usually used in the industry, which is added to the water in which the olives are found (this method should not be used at home if we had olive trees because soda is highly corrosive and very dangerous, in this case we should use table salt). Normally 1 kilogram of soda is added for every 3 liters of water (weighing 3 kg, remember that the density of water is 1 g/mL).Thus, 4 kg of solution were obtained, and the density of this solution was determined experimentally to be 1.25 g/mL. a) Calculate what volume of solution is obtained. (Remember that d = m/V). b) What will be the concentration of that solution expressed in grams of solute dissolved in each liter of solution? c) What will be the concentration expressed in % by mass (or weight)? • If we separate a ladle (100 mL) of that solution. d) What will be the concentration of soda in the liquid in the ladle? e) How many grams of…

What is the normality of a solution made by dissolving 10.00 g of hydrogen phosphate, H3PO4 in water to a volume of 150 mL? Note: Please present complete solution. Express your final answers up to two (2) decimal places.

A chemist must dilute 21.1mL of 6.81M aqueous calcium bromide CaBr2 solution until the concentration falls to 2.00M. He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in milliliters. Round your answer to 3 significant digits.

An aqueous sodium nitrate (NANO3) solution must be created for an experiment. If 50.00 mL of a 0.150 M solution is needed, what amount of sodium nitrate (in grams) must be weighed out? Only input numbers. Your answers must be expressed to the thousandths place. Any values less than one must have a zero in front of the decimal (e.g. 0.01 not .01).

A solution containing 78 g of NaNO3 in 70. g H2O at 50 ° C is cooled to 20 °C. Use the solubility data from the table below. Part A Solubility (g/100. g H2O) Substance 20 °C 50 °C How many grams of NaNO3 remain in solution at 20 °C? KCI 34 43 Express your answer in grams to two significant figures. NaNO3 88 110 ? C12 H22O11 (sugar) 204 260

A student prepares a 0.28 mM aqueous solution of acetic acid (CH,CO,H). Calculate the fraction of acetic acid that is in the dissociated form in his solution. Express your answer as a percentage. You will probably find some useful data in the ALEKS Data resource. Round your answer to 2 significant digits. |% x10