14. Solutions

Parts per Million (ppm)

Solution Concentration: Parts Per Million

Most fish need at least 4 ppm dissolved O2 in water for survival. (a) What is this concentration in mol>L?

Parts Per Million (ppm) and Parts Per Billion (ppb) - Solution Concentration

(b) Concentrations of lead in the bloodstream are often quoted in units of μg/dL. Averaged over the entire country, the mean concentration of lead in the blood was measured to be 1.6 μg/dL in 2008. Express this concentration in ppb.

Phosphorus is present in seawater to the extent of 0.07 ppm by mass. Assuming that the phosphorus is present as dihydrogenphosphate, H2PO4-, calculate the correspond-ing molar concentration of H2PO4- in seawater.

The Safe Drinking Water Act (SDWA) sets a limit for mercury—a 
toxin to the central nervous system—at 0.0020 ppm by mass. 
Water suppliers must periodically test their water to ensure that 
mercury levels do not exceed this limit. Suppose water becomes 
contaminated with mercury at twice the legal limit (0.0040 
ppm). How much of this water would a person have to consume 
to ingest 50.0 mg of mercury?

A water sample contains the pollutant chlorobenzene with a concentration of 16 ppm (by volume). What volume of this water contains 5.01×102 mL of chlorobenzene?

SOLUTIONS - Concentration in PARTS PER MILLION (ppm) & PARTS PER BILLION (ppb) | Chemistry with Cat

Parts per Million (ppm) Example 1

Which of the following solutions has the higher molarity? (a) 10 ppm KI in water or 10,000 ppb KBr in water

Fluoride ion is added to drinking water at low concentra- tions to prevent tooth decay. What mass of sodium fluoride (NaF) should be added to 750 L of water to make a solution
that is 1.5 ppm in fluoride ion? (LO 13.5) (a) 1.1 g (b) 2.5 g (c) 0.51 g (d) 3.1 g

How would you prepare each of the following solutions? (a) 100 mL of a 155 ppm solution of urea, CH4N2O, in water

How to Measure Parts Per Million in Chemistry : Solving Math Problems

Federal regulations set an upper limit of 50 parts per million
(ppm) of NH3 in the air in a work environment [that is, 50
molecules of NH31g2 for every million molecules in the air].
Air from a manufacturing operation was drawn through a
solution containing 1.00 * 102 mL of 0.0105 M HCl. The
NH3 reacts with HCl according to:
NH31aq2 + HCl1aq2¡NH4Cl1aq2
After drawing air through the acid solution for 10.0 min at a
rate of 10.0 L/min, the acid was titrated. The remaining acid
needed 13.1 mL of 0.0588 M NaOH to reach the equivalence
point. (a) How many grams of NH3 were drawn into the
acid solution?

Parts per Million (ppm) Example 2

The average human body contains about 5,000 grams of blood. What mass of arsenic is present in the body if the amount in blood is 0.86 ppb?

A 5.12 L sample of solution contains 0.230 g of potassium sulfate, K2SO4. Determine the concentration of K2SO4 in ppm if the density of the solution is 1.30 g/mL.

Calculate ppm for a solution (parts per million) using formula

The ozone layer in the Earth’s stratosphere has an average total pressure of 10 mm Hg 11.3 * 10-2 atm2. The partial pressure of ozone in the layer is about 1.2 * 10-6 mm Hg
11.6 * 10-9 atm2. What is the concentration of ozone in
parts per million, assuming that the average molar mass of
air is 29 g/mol?

Parts per Million (ppm) Concept 1

Calculate the concentration in parts per billion of the following aqueous solution:0.91 mg of caffeine in a total volume of 131 mL.

Parts per Million (ppm) Concept 2

An impurity in water has an extinction coefficient of 3.45 * 103 M-1 cm-1 at 280 nm, its absorption maximum (A Closer Look, p. 576). Below 50 ppb, the impurity is not a problem for human health. Given that most spectrome- ters cannot detect absorbances less than 0.0001 with good reliability, is measuring the absorbance of a water sample at 280 nm a good way to detect concentrations of the impu- rity above the 50-ppb threshold?

Federal regulations set an upper limit of 50 parts per million
(ppm) of NH3 in the air in a work environment [that is, 50
molecules of NH31g2 for every million molecules in the air].
Air from a manufacturing operation was drawn through a
solution containing 1.00 * 102 mL of 0.0105 M HCl. The
NH3 reacts with HCl according to:
NH31aq2 + HCl1aq2¡NH4Cl1aq2
After drawing air through the acid solution for 10.0 min at a
rate of 10.0 L/min, the acid was titrated. The remaining acid
needed 13.1 mL of 0.0588 M NaOH to reach the equivalence
point. (b) How many ppm of NH3 were in the air?
(Air has a density of 1.20 g/L and an average molar mass of
29.0 g>mol under the conditions of the experiment.)

The maximum allowable concentration of lead in drinking
water is 9.0 ppb. (b) How many grams of lead are in a swimming pool containing 9.0 ppb lead in 60 m3 of water?

Glucose makes up about 0.102% by mass of human blood. Calculate this concentration in ppm.

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[BOOK CHEM] Clutch Version

Types of Aqueous Solutions

When an ionic solid dissolves, ions leave the solid and become dispersed in the solvent. Three possible aqueous solutions can be formed:saturated, unsaturated and supersaturated.

Boiling Point Elevation

Boiling Point Elevation is the phenomenon when adding a solute to a pure solvent results in increased boiling point of the solvent.

Intro to Henry's Law

According to&nbsp;Henry's Law, at a constant temperature the amount of a gas dissolved in a solvent is directly proportional to its partial pressure when it is in equilibrium with its liquid phase.&nbsp;

Osmotic Pressure

Osmotic Pressure is the force that drives Osmosis from higher concentration to lower concentration.

Mole Fraction

Mole Fraction (X) relates the moles of solute and solvent within a solution.&nbsp;

The Colligative Properties

The&nbsp;Colligative Properties&nbsp;explain what happens to a pure solvent as it transitions to a solution.

Molality

Molality (m)&nbsp;represents the number of moles of solute dissolved per kilogram of solvent.&nbsp;

Freezing Point Depression

Freezing Point Depression is the phenomenon when adding a solute to a pure solvent results in decreased freezing point of the solvent.

Solutions: Solubility and Intermolecular Forces

Solutions are homogeneous mixtures that result from the dissolving of a solute by a solvent.

Vapor Pressure Lowering (Raoult's Law)

Vapor Pressure is the pressure exerted by a gas at equilibrium with its liquid phase at a specific temperature in a closed system.

Henry's Law Calculations

To calculate solubility of a dissolves gas, Henry's Law Constant and partial pressure are used.

Solutions: Mass Percent

Mass Percent represents grams of solute per grams of solution, multiplied by 100.

Osmosis

Osmosis is the net movement of solvent across a semipermeable membrane.

<div dir="auto"><div contenteditable="true"dir="auto"spellcheck="true">Parts per Million (ppm) and Parts per Billion (ppb) are used to express extremely dilute solution concentrations.</div></div>

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