Login

Search the forums now!

Welcome, Guest. Please login or register.

November 01, 2025, 12:43:07 pm
Pages: [1]   Go Down

Author Topic: Simple concentration question  (Read 1310 times)  Share 

0 Members and 1 Guest are viewing this topic.

dekoyl

  • Victorian
  • ATAR Notes Superstar
  • ******
  • Posts: 2152
  • Respect: +18
Simple concentration question
« on: December 25, 2008, 01:15:57 am »
0
For a 0.20M solution of potassium sulfate, calculate the amount, in mol, of:
a) Potassium ions,

The answer does this as first step:
a)   n(K2SO4) = C × V = 0.20 × 0.250 = 0.050 mol

I think M was mol/L but why is V 250mL in this case?

Thanks.
Logged

vce08

  • Guest
Re: Simple concentration question
« Reply #1 on: December 25, 2008, 01:17:33 am »
0
i think you forgot to tell us some info
Logged

shinny

  • VN MVP 2010
  • Honorary Moderator
  • ATAR Notes Legend
  • *******
  • Posts: 4327
  • Respect: +256
  • School: Melbourne High School
  • School Grad Year: 2008
Re: Simple concentration question
« Reply #2 on: December 25, 2008, 01:18:13 am »
0
Someone else already asked this somewhere. Long story cut short; the question is screwed up.
Logged
MBBS (hons) - Monash University

YR11 '07: Biology 49
YR12 '08: Chemistry 47; Spesh 41; Methods 49; Business Management 50; English 43

ENTER: 99.70

hard

  • Guest
Re: Simple concentration question
« Reply #3 on: December 25, 2008, 01:18:33 am »
0
Quote from: dekoyl on December 25, 2008, 01:15:57 am
For a 0.20M solution of potassium sulfate, calculate the amount, in mol, of:
a) Potassium ions,

The answer does this as first step:
a)   n(K2SO4) = C × V = 0.20 × 0.250 = 0.050 mol

I think M was mol/L but why is V 250mL in this case?

Thanks.
that's weird, you must've not read the question properly i mean the volume cannot be just made up.
ehhh i'm still revising a bit of unit 1/2 chemistry. FUCK MID YEAR IS SO CLOSE!
Logged

dekoyl

  • Victorian
  • ATAR Notes Superstar
  • ******
  • Posts: 2152
  • Respect: +18
Re: Simple concentration question
« Reply #4 on: December 25, 2008, 01:20:07 am »
0
Quote from: hard on December 25, 2008, 01:18:33 am
FUCK MID YEAR IS SO CLOSE!
Oh shut up, mate. I hate hearing stuff like that :P Please don't get me nervous

Quote from: shinny on December 25, 2008, 01:18:13 am
Someone else already asked this somewhere. Long story cut short; the question is screwed up.
Ah thanks shinny =O
Logged

AQ

  • Victorian
  • Trendsetter
  • **
  • Posts: 167
  • Me when 5yrs old.
  • Respect: +1
Re: Simple concentration question
« Reply #5 on: December 30, 2008, 08:58:59 pm »
0
Quote from: hard on December 25, 2008, 01:18:33 am
Quote from: dekoyl on December 25, 2008, 01:15:57 am
For a 0.20M solution of potassium sulfate, calculate the amount, in mol, of:
a) Potassium ions,

The answer does this as first step:
a)   n(K2SO4) = C × V = 0.20 × 0.250 = 0.050 mol

I think M was mol/L but why is V 250mL in this case?

Thanks.
that's weird, you must've not read the question properly i mean the volume cannot be just made up.
ehhh i'm still revising a bit of unit 1/2 chemistry. FUCK MID YEAR IS SO CLOSE!

mid year is close?
Lol, i totally forgot about it.
Logged
2008: | Further (39) |
2009: | Methods (35+) | Chem (35+) | English (33+) | 
Last two: [| Accounting (34+) | Legal (34+)]  
ENTER: 85+

2010: | Architecture @ UOM or Civil at RMIT |


Ne mutlu TURKUM Diyene

khalil

  • Guest
Re: Simple concentration question
« Reply #6 on: December 30, 2008, 09:20:56 pm »
0
Quote from: AQ on December 30, 2008, 08:58:59 pm
Quote from: hard on December 25, 2008, 01:18:33 am
Quote from: dekoyl on December 25, 2008, 01:15:57 am
For a 0.20M solution of potassium sulfate, calculate the amount, in mol, of:
a) Potassium ions,

The answer does this as first step:
a)   n(K2SO4) = C × V = 0.20 × 0.250 = 0.050 mol

I think M was mol/L but why is V 250mL in this case?

Thanks.
that's weird, you must've not read the question properly i mean the volume cannot be just made up.
ehhh i'm still revising a bit of unit 1/2 chemistry. FUCK MID YEAR IS SO CLOSE!

mid year is close?
Lol, i totally forgot about it.
Midyear will be a breeze. Its the end of year exams that are critical!
Logged
Pages: [1]   Go Up