Answer:
0.0428 M
Explanation:
Because we're asked to calculate the molarity of nickel(II) cation, we need to <u>determine all sources for that species</u>, in this case, all Ni⁺² comes from the nickel(II) bromide solid (NiBr₂).
We use the molecular weight of NiBr₂ to calculate the moles of Ni:
1.87 g NiBr₂ ÷ 218.49g/mol * (1molNi⁺²/1molNiBr₂) = 8.55x10⁻³ mol Ni⁺²
Then we <u>divide the moles by the volume in order to calculate the concentration</u>:
8.55x10⁻³ mol Ni⁺² / 0.200 L = 0.0428 M
What are the answers you can pick
Answer:
Explanation:
Given data:
A) Moles of H₂O₂ = 7.00
Mass of H₂O₂ = ?
Solution:
Number of moles = mass/ molar mass
Now we will rearrange this formula:
Mass = Number of moles × molar mass
Mass = 7.00 mol × 34 g/mol
Mass = 238 g
B) Moles of NaOH = 5.60 mol
Mass of NaOH = ?
Solution:
Number of moles = mass/ molar mass
Now we will rearrange this formula:
Mass = Number of moles × molar mass
Mass = 5.60 mol × 40 g/mol
Mass = 224 g
C) Moles of Ca(CN)₂ = 0.780
Mass of Ca(CN)₂ = ?
Solution:
Number of moles = mass/ molar mass
Now we will rearrange this formula:
Mass = Number of moles × molar mass
Mass = 0.780 mol × 92.11 g/mol
Mass = 71.85 g
Answer: Most of the volume of a gas is composed of the large amounts of empty space between the gas particles.
Explanation:
Answer: <u>Mixtures can be physically separated but pure substances cannot be physically separated.</u>
Explanation: Mixtures can be physically separated by using methods that use differences in physical properties to separate the components of the mixture, such as evaporation, distillation, filtration and chromatography. A pure substance, any compound or element, can't be separated into different atoms by physical methods. Pure substances are compounds and elements (made up of the same atom or same molecule respectively), while mixtures are an assortment of different substances put together. Hope this helps ^-^.