how many grams of HCL scid is needed to make vessel-2 compelety neutral
Answers
Answer:
Molarity
The most common unit of solution concentration is molarity (M).
The molarity of a solution is defined as the number of moles of
solute per one liter of solution. Note that the unit of volume for
molarity is liters, not milliliters or some other unit. Also note
that one liter of solution contains both the solute and the solvent.
Molarity, therefore, is a ratio between moles of solute and liters of
solution. To prepare laboratory solutions, usually a given volume
and molarity are required. To determine molarity, the formula
weight or molar mass of the solute is needed. The following examples illustrate the calculations for preparing solutions.
If starting with a solid, use the following procedure:
• Determine the mass in grams of one mole of solute, the molar
mass, MMs.
• Decide volume of solution required, in liters, V.
• Decide molarity of solution required, M.
• Calculate grams of solute (gs) required using equation 1.
eq. 1. gs = MMs x M x V
• Example: Prepare 800 mL of 2 M sodium chloride.
(MMNaCl = 58.45 g/mol)
gNaCl = 58.45 g/mol x 2 mol/L x 0.8 L
gNaCl = 93.52 g NaCl
Dissolve 93.52 g of NaCl in about 400 mL of distilled water,
then add more water until final volume is 800 mL.
If starting with a solution or liquid reagent:
• When diluting more concentrated solutions, decide what
volume (V2) and molarity (M2) the final solution should be.
Volume can be expressed in liters or milliliters.
Basic Concepts of Preparing Solutions
Many of the reagents used in science are in the form of solutions
which need to be purchased or prepared. For many purposes, the exact
value of concentration is not critical; in other cases, the concentration
of the solution and its method of preparation must be as accurate as
possible. The Flinn Laboratory Solution Preparation reference section
is designed for both the novice and experienced solution maker. It
provides valuable information on the basic concepts of preparing solutions and instructions for preparing most solutions required in the high
school science laboratory. Professional quality solutions are possible
when high quality and fresh chemicals and solvents are used, and
meticulous procedures are followed. Many of the solutions described
• Basic concepts of preparing
solutions
• Over 300 recipes of common
laboratory solutions
• Solution preparation tips
Laboratory Solution
Preparation
in this section are available ready-made from Flinn Scientific to save
valuable laboratory prep time.
The section is divided into several parts for your convenience.
Basic concepts of preparing solutions
Preparation of simple inorganic salt solutions
Preparations of acid and base solutions
Recipes for Biological, Histological, and Chemical solutions
• Determine molarity (M1) of starting, more concentrated solution.
• Calculate volume of starting solution (V1) required using equation 2. Note: V1 must be in the same units as V2.
eq. 2. M1V1 = M2V2
• Example: Prepare 100 mL of 1.0 M hydrochloric acid from
concentrated (12.1 M) hydrochloric acid.
M1V1 = M2V2
(12.1 M)(V1) = (1.0 M)(100 mL)
V1 = 8.26 mL conc. HCl
Add 8.26 mL of concentrated HCl to about 50 mL of distilled
water, stir, then add water up to 100 mL.
Percent Solutions
Mass percent solutions are defined based on the grams of solute
per 100 grams of solution.
Example: 20 g of sodium chloride in 100 g of solution is a 20%
by mass solution.
Volume percent solutions are defined as milliliters of solute per
100 mL of solution.
Example: 10 mL of ethyl alcohol plus 90 mL of H2O (making
approx. 100 mL of solution) is a 10% by volume
solution.
Mass-volume percent solutions are also very common. These
solutions are indicated by w/v% and are defined as the grams of
solute per 100 milliliters of solution.
Example: 1 g of phenolphthalein in 100 mL of 95% ethyl
alcohol is a 1 w/v% solution.
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