Using moles, volume in dm 3 and concentration, complete the equation: Moles = (Higher tier only)

Using moles, volume in dm 3 and concentration, the equation is: Moles = concentration x volume

Calculate the number of moles of solute present in 2.0 dm 3 of a solution whose concentration is 0.15 mol dm -3 . (Higher tier only)

To calculate the number of moles of solute present in 2.0 dm 3 of a solution whose concentration is 0.15 mol dm -3 : Moles = concentration x volume Moles = 0.15 x 2.0 = 0.3 moles

What are the two common units for concentration? (Higher tier only)

The two common units for concentration are: g / dm 3 mol / dm 3

State the equation for concentration using moles and volume. (Higher tier only)

The equation for concentration using moles and volume is: concentration = moles / volume

What is the concentration of a solution where 1.0 mole of solute is dissolved in 2.0 dm 3 of water? (Higher tier only)

The concentration of a solution where 1.0 mole of solute is dissolved in 2.0 dm 3 of water is: Concentration = moles / volume Concentration = 1.0 / 2.0 = 0.5 mol dm -3

How do you calculate the volume of a solution using moles and concentration? (Higher tier only)

The equation to calculate the volume of a solution using moles and concentration is: Volume = moles / concentration

Using volume in dm 3 and concentration, complete the equation: Moles = (Higher tier only)

Using moles, volume in dm 3 and concentration, the equation is: Moles = concentration x volume

Calculate the number of moles in 2.5 dm 3 of a solution that has a concentration of 0.30 mol dm -3 . (Higher tier only)

To calculate the number of moles present in 2.5 dm 3 of a solution which has a concentration of 0.30 mol dm -3 : Moles = concentration x volume Moles = 0.30 x 2.5 = 0.75 moles

What are the four steps to solve a titration calculation? (Higher tier only)

The four steps in a titration calculation are: Write out the balanced equation for the reaction Calculate the moles of the known solution given the volume and concentration Use the equation to deduce the moles of the unknown solution Use the moles and volume of the unknown solution to calculate the concentration

Explain how many moles of HCl will be neutralised by 0.05 moles of NaOH. HCl + NaOH → NaCl + H 2 O (Higher tier only)

0.05 moles of HCl would be required as this reaction is a 1:1 ratio.

GCSEChemistryAQAFlashcardsQuantitative ChemistryConcentration of Solutions

Concentration of Solutions (AQA GCSE Chemistry)

Flashcards

1/14

FrontUsing Concentrations in mol/dm3
Using moles, volume in dm³ and concentration, complete the equation:
Moles =
(Higher tier only)
FrontUsing Concentrations in mol/dm3
Calculate the number of moles of solute present in 2.0 dm³ of a solution whose concentration is 0.15 mol dm^-3.
(Higher tier only)
BackUsing Concentrations in mol/dm3
To calculate the number of moles of solute present in 2.0 dm³ of a solution whose concentration is 0.15 mol dm^-3:
Moles = concentration x volume
Moles = 0.15 x 2.0 = 0.3 moles
FrontUsing Concentrations in mol/dm3
What are the two common units for concentration?
(Higher tier only)
BackUsing Concentrations in mol/dm3
The two common units for concentration are:
g / dm³
mol / dm³

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Cards in this collection (14)

Using moles, volume in dm³ and concentration, complete the equation:
Moles =
(Higher tier only)
Using moles, volume in dm³ and concentration, the equation is:
Moles = concentration x volume
Calculate the number of moles of solute present in 2.0 dm³ of a solution whose concentration is 0.15 mol dm^-3.
(Higher tier only)
To calculate the number of moles of solute present in 2.0 dm³ of a solution whose concentration is 0.15 mol dm^-3:
- Moles = concentration x volume
- Moles = 0.15 x 2.0 = 0.3 moles
What are the two common units for concentration?
(Higher tier only)
The two common units for concentration are:
- g / dm³
- mol / dm³
State the equation for concentration using moles and volume.
(Higher tier only)
The equation for concentration using moles and volume is:
concentration = moles / volume
What is the concentration of a solution where 1.0 mole of solute is dissolved in 2.0 dm³ of water?
(Higher tier only)
The concentration of a solution where 1.0 mole of solute is dissolved in 2.0 dm³ of water is:
- Concentration = moles / volume
- Concentration = 1.0 / 2.0 = 0.5 mol dm^-3
How do you calculate the volume of a solution using moles and concentration?
(Higher tier only)
The equation to calculate the volume of a solution using moles and concentration is:
Volume = moles / concentration
Using volume in dm³ and concentration, complete the equation:
Moles =
(Higher tier only)
Using moles, volume in dm³ and concentration, the equation is:
Moles = concentration x volume
Calculate the number of moles in 2.5 dm³ of a solution that has a concentration of 0.30 mol dm^-3.
(Higher tier only)
To calculate the number of moles present in 2.5 dm³ of a solution which has a concentration of 0.30 mol dm^-3:
- Moles = concentration x volume
- Moles = 0.30 x 2.5 = 0.75 moles
What is 27.50 cm³ in dm³?
(Higher tier only)
27.50 cm³ is 0.0275 dm³.
A solution of HCl has a volume of 23.55 cm³ and contains 0.00375 moles. What is its concentration in mol/dm³?
(Higher tier only)
The concentration in mol/dm³ of a solution of HCl with a volume of 23.55 cm³ and contains 0.00375 moles is:
- Volume in dm³ = 0.02355 dm³
- Concentration = $\frac{0.00375}{0.02355}$ = 0.16 mol/dm³
What are the four steps to solve a titration calculation?
(Higher tier only)
The four steps in a titration calculation are:
1. Write out the balanced equation for the reaction
2. Calculate the moles of the known solution given the volume and concentration
3. Use the equation to deduce the moles of the unknown solution
4. Use the moles and volume of the unknown solution to calculate the concentration
Using moles and volume in dm³, complete the equation:
Concentration =
(Higher tier only)
Using moles, volume in dm³ the equation is:
Concentration = $\frac{moles}{volume}$
What is 0.03905 dm³ in cm³?
(Higher tier only)
0.03905 dm³ is 39.05 cm³.
Explain how many moles of HCl will be neutralised by 0.05 moles of NaOH.
HCl + NaOH → NaCl + H₂O
(Higher tier only)
0.05 moles of HCl would be required as this reaction is a 1:1 ratio.

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