Lexi
Lexi asked in Science & MathematicsChemistry · 3 years ago

Possible set of Quantum Numbers for 5p?

This is from a set of practice problems for general chemistry 1 and I thought it could be narrowed down to B, C, and D but I don't know where to go from there

A possible set of quantum numbers to describe an electron in a 5p subshell is

A) n = 3, l = 1, ml = 1, ms = - 1/2

B) n = 5, l = 1, ml = 0, ms = +1/2

C) n = 4, l = 0, ml = 0, ms = - 1/2

D) n = 5, l = 2, ml = 2 , ms = +1/2

E) n = 5, l = 0, ml = 0, ms = +1/2

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1 Answer

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  • akihiko
    Lv 4
    3 years ago

    5p; n=5, L=1, m=1, s=-1/2

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Jaybirdy
Jaybirdy asked in Science & MathematicsChemistry · 9 years ago

How to make a 0.1M solution?

I have been asked what mass of potassium hydrogenphthalate will be needed to make a 250cm3 of 0.1M??

If someone could right out how to do this, so i know for the future. Thanks

How to make a 0.1M solution?

7 Answers

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  • Anonymous
    9 years ago
    Best Answer

    potassium hydrogen phthalate has formula KHC8H4O4 and it's molar mass is 204.23 grams

    To make a 0.1 molar solution you need to understand what molarity is.

    Molarity = moles of solute/ volume of solution in liters

    0.1 M = 0.1 moles of KHC8H4O4 in a litre of water

    or 0.025 moles of KHC8H4O4 in 250 ml of water ( assuming 1 cm3 = 1 ml)

    So you need 0.025 moles of KHC8H4O4 to be dissolved completely in 250 ml of water.

    Therefore Mass required = 0.025 x 204.23 = 5.1 grams ( approx.)

    Hope this helps:-)

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  • Charlie
    9 years ago

    A 0.1M solution means 0.1 moles per Liter of solution. Perform a dimensional analysis

    0.1mol/L * 250 mL * 1 L / 1000 mL = ___ --> this would give the moles of KHP you need. Multiply this by molecular weight (grams/mole) so that you'll get the necessary mass of KHP

    Source(s): Basic Chem stock knowledge
  • None
    Lv 7
    9 years ago

    1/40 of the molecular weight of KHP in 250 ml of solution is a 0.1M solution

    Potassium hydrogen phthalate (KHP) is a salt of phthalic acid in which one of the hydrogens has been replaced by potassium. Find the MW by checking:

    http://en.wikipedia.org/wiki/Potassium_hydrogen_ph...

  • dorthy
    Lv 4
    3 years ago

    0.1 Molar Solution

    Source(s): https://owly.im/a9jZw
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  • Umar
    Lv 7
    9 years ago

    KHP has a molar mass of 204.227g/mol. So 0.10M = 20.4227g/L = 5.1057g in 250mL.

    So you need to weigh 5.1057g of the salt and dissolve it into a 250ml volumetric flask and then dilute to the mark.

  • Ramesh Chandra
    5 years ago

    pyrogall 0.1 M solution

  • Khurram
    5 years ago

    Ferrous chloride (iron(II) chloride) solution

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Anonymous
Anonymous asked in Science & MathematicsChemistry · 1 decade ago

I have 1 gallon of 31.5% HCL - How much of this solution (in ml) is equal to 2 Moles HCL?

and how do you figure that out?

Update:

(that is 31.5% HCL in H2O(water))

I have 1 gallon of 31.5% HCL - How much of this solution (in ml) is equal to 2 Moles HCL?

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  • Trevor H
    Lv 7
    1 decade ago
    Best Answer

    Without proper details, these % problems are often guesswork. I can assume that by a 31.5% HCl solution you refer to 31.5g HCl in 100ml water. ( based on you using volumes in the question). There are other ways of interpreting a 31.5% solution, which will result in a different answer.

    2mol HCl = 2*(1.008+35.453) = 72.922g HCl

    100ml = 31.5g HCl

    72.922g HCl = 72.922/31.5*100 = 231.5ml

    If you measure out 231.5ml of the acid solution, you will have 2mol HCl

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blue16
blue16 asked in Science & MathematicsChemistry · 8 years ago

Partial Pressure Problem?

The total pressure of a system that contains NH3(g) and Ne(g) is 655 mmHg. If the mass of NH3 is triple the mass of Ne, calculate the partial pressure of NH3 assuming no reaction in the container.

Partial Pressure Problem?

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  • Lexi R
    Lv 7
    8 years ago
    Best Answer

    partial pressure of a gas = mole fraction of that gas x total volume

    we know that the mass of NH3 is 3x the mass of Ne, we can use this to determine the mole fraction of NH3

    eg, If mass Ne = 10 g

    mass NH3 = 30 g

    moles Ne = mass / molar mass = 10 g / 20.18 g/mol = 0.49554 mol

    moles NH3 = 30 g / 17.034 g/mol = 1.76118 mol

    total moles = 0.49554 mol + 1.76118 mol = 2.25672 mol

    mole fraction NH3 = moles NH3 / total moles

    = 1.76118 mol / 2.25672 mol

    = 0.7804

    partial pressure NH3 = mole fraction NH3 x total pressure

    = 0.7804 x 655 mmHg

    = 511.162 mmHg

    = 511 mmHg (3 sig figs)

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