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Unit 5 – Ionic Bonding

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SOLUTIONS- STUDENT EXERCISE
CALCULATING CONCENTRATION - MOLARITY
1. Calculate the Molarity of the solution.
a. 2 moles of KF in 1 liter of water (2 moles/liter)
π‘€π‘œπ‘™π‘Žπ‘Ÿπ‘–π‘‘π‘¦ = 𝑀 =
π‘šπ‘œπ‘™π‘’π‘  π‘œπ‘“ π‘ π‘œπ‘™π‘’π‘‘π‘’
2 π‘šπ‘œπ‘™π‘’π‘ 
π‘šπ‘œπ‘™π‘’π‘ 
=
=2
= 2𝑀
π‘™π‘–π‘‘π‘’π‘Ÿπ‘  π‘œπ‘“ π‘ π‘œπ‘™π‘’π‘‘π‘–π‘œπ‘›
1 π‘™π‘–π‘‘π‘’π‘Ÿ
π‘™π‘–π‘‘π‘’π‘Ÿ
b. 58 grams of KF in 1 liter of water ( 1 mile/liter) (first calculate MM and then the number of
moles)
Molar Mass of KF: 1 (39 g/mole) + 1 (19 g/mole ) = 58 grams/mole
Convert Mass to Moles:
πŸ“πŸ– π’ˆπ’“π’‚π’Žπ’”
𝟏
𝟏 π’Žπ’π’π’†
× πŸ“πŸ– π’ˆπ’“π’‚π’Žπ’” = 𝟏 π’Žπ’π’π’† 𝒐𝒇 𝑲𝑭
Calculate Molarity:
π‘€π‘œπ‘™π‘Žπ‘Ÿπ‘–π‘‘π‘¦ = 𝑀 =
π‘šπ‘œπ‘™π‘’π‘  π‘œπ‘“ π‘ π‘œπ‘™π‘’π‘‘π‘’
1 π‘šπ‘œπ‘™π‘’π‘ 
π‘šπ‘œπ‘™π‘’π‘ 
=
=1
= 1𝑀
π‘™π‘–π‘‘π‘’π‘Ÿπ‘  π‘œπ‘“ π‘ π‘œπ‘™π‘’π‘‘π‘–π‘œπ‘›
1 π‘™π‘–π‘‘π‘’π‘Ÿ
π‘™π‘–π‘‘π‘’π‘Ÿ
c. 75 grams of CaCl2 in 1 liter of water ( .67 mile/liter)
Molar Mass of CaCl2: 1 (40 g/mole) + 2 (35.5 g/mole ) = 111 grams/mole
Convert Mass to Moles:
πŸ•πŸ“ π’ˆπ’“π’‚π’Žπ’”
𝟏
𝟏 π’Žπ’π’π’†
× πŸπŸπŸ π’ˆπ’“π’‚π’Žπ’” =. πŸ”πŸ• π’Žπ’π’π’† 𝒐𝒇 π‘ͺ𝒂π‘ͺπ’πŸ
Calculate Molarity:
π‘€π‘œπ‘™π‘Žπ‘Ÿπ‘–π‘‘π‘¦ = 𝑀 =
π‘šπ‘œπ‘™π‘’π‘  π‘œπ‘“ π‘ π‘œπ‘™π‘’π‘‘π‘’
. 67 π‘šπ‘œπ‘™π‘’π‘ 
π‘šπ‘œπ‘™π‘’π‘ 
=
= .67
= .67 𝑀
π‘™π‘–π‘‘π‘’π‘Ÿπ‘  π‘œπ‘“ π‘ π‘œπ‘™π‘’π‘‘π‘–π‘œπ‘›
1 π‘™π‘–π‘‘π‘’π‘Ÿ
π‘™π‘–π‘‘π‘’π‘Ÿ
d. 43.5 grams of LiBr in .4 liters of water
Molar Mass of LiBr: 1 (7 g/mole) + 1 (80 g/mole ) = 87 grams/mole
Convert Mass to Moles:
πŸ’πŸ‘.πŸ“ π’ˆπ’“π’‚π’Žπ’”
𝟏
𝟏 π’Žπ’π’π’†
× πŸ–πŸ•π’ˆπ’“π’‚π’Žπ’” =. πŸ“ π’Žπ’π’π’† 𝒐𝒇 π‘³π’Šπ‘©π’“
Calculate Molarity:
π‘€π‘œπ‘™π‘Žπ‘Ÿπ‘–π‘‘π‘¦ = 𝑀 =
π‘šπ‘œπ‘™π‘’π‘  π‘œπ‘“ π‘ π‘œπ‘™π‘’π‘‘π‘’
. 5 π‘šπ‘œπ‘™π‘’π‘ 
π‘šπ‘œπ‘™π‘’π‘ 
=
= 1.25
= 1.25 𝑀
π‘™π‘–π‘‘π‘’π‘Ÿπ‘  π‘œπ‘“ π‘ π‘œπ‘™π‘’π‘‘π‘–π‘œπ‘›
. 4 π‘™π‘–π‘‘π‘’π‘Ÿ
π‘™π‘–π‘‘π‘’π‘Ÿ
CALCULATING # of Moles
2. Calculate the number of moles in the following questions.
a. How many moles of HCl are in .5 liters of a 1 Molar solution of HCl? (.5 moles)
b. How many moles of NaCl are in 10 liters of a .1 Molar solution of NaCl? ( 1 mole)
c. How many moles of KI are in .75 liters of a 1.25 Molar solution of KI? (.9375 moles)
CALCULATING VOLUME (# of Liters)
3. Calculate the number of liters for the following questions
a. How many liters of a .1 Molar solution NaCl are necessary to have 1 mole of NaCl? (10 liters)
b. How many liters of a 1.25 Molar solution KI are necessary to have .9375 moles of KI? (.75
liters)

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