Question

The final buret reading in ml is 31.12
The initial buret reading in ml is 15.72
The volume of titrant in ml is 15.49

what is the moles of NAOH used?

Answer 1

@Somy

Answer 2

This is actually something I'm in the middle of learning, so I wouldn't know. Sorry.

Answer 3

Do you have an equation to go with it?

Answer 4

The final buret reading in ml is 31.12
The initial buret reading in ml is 15.72
The volume of titrant in ml is 15.49

Answer 5

and they told us to find the moles of NAOH used

Answer 6

31.12- 15.72 = 15.4

Assuming NaOH is in the burette [seriously? -.-], relative molecular mass of NaOH is 23+16+1 = 40

Answer 7

volume of titrant is 15.49 ml. They didn't even give you the molarity? Concentration?

Answer 8

Do you have a molarity of either or the solutions?

Answer 9

what solutions are you titrating?

Answer 10

The final buret reading in ml is 31.12
The initial buret reading in ml is 15.72
The volume of titrant in ml is 15.49

what is the moles of NAOH used?

Answer 11

molarity of standarized NAOH solution is 0.1012 M

Answer 12

Convert your ml of naoh solution used to litters.

Answer 13

Sorry i havent done this yet

Answer 14

then multiply it to the .1012

Answer 15

\[\frac{moles}{Litters}*Litters=moles\]

Answer 16

no

\[Molarity=\frac{moles}{Litters}\]

Answer 17

So for this problem

\[\frac{.1012 moles}{L}*.001549 L = x moles\]

Answer 18

check the conversion of ml to litters

Answer 19

0.0001012 is that the litter

Answer 20

it looks like you divided the molarity by a thousand when you should have divided the volume reading from the buret

Answer 21

they also gave me this in the probelm. volume of dilluted vingar used in each titration is 20 mL .02 L

Answer 22

look at the units you want moles. you have a molarity and a volume of titrant used. if you convert the titrant from ml to L and multiply them together you can get moles by from the information provided by the problem.

Answer 23

i don't getr it

Answer 24

I told you this is not fresh in my mind.

you first need to balance the equation.
you know the mass of one mole.
set up the ratio with the volume

Answer 25

tha is the equation

Answer 26

Molarity=moles/Litters

Answer 27

moles/Litters*Litters=moles

Answer 28

1012moles/L*.001549L=xmoles

Answer 29

Sigh... are you kidding me. General Titration? I'm really not willing to help on this one, but @nincompoop is. COUGH COUGH

Answer 30

what is the moles of NAOH used?


Use: \(\sf Molarity_{NaOH} =\dfrac{moles~of~NaOH}{Liters~of~NaOH}\)

Molarity=0.1012 M
volume=15.49 mL = 0.01549 L

plug and solve

Answer 31

is is .1012/.001549 = 65.33

Answer 32

no using the formula just given by @aaronq Molarity = moles/volume to get moles you would multiply the molarity by the volume to get moles not divide

Answer 33

is it .001567588

Answer 34

yes it is !

\(\sf Molarity=\dfrac{moles}{L}\rightarrow moles=moles*Molarity=0.01549 L*0.1012 M\)

moles=0.001567588 mol

Answer 35

crap i meant liters*molarity in the formula

Answer 36

so should i put .001567588 as answer

Answer 37

asit says how many moles

Answer 38

nope, you wanna round that up, maybe even use scientific notation

Answer 39

All your values have 4 sig figs, so you wanna keep 4 sig figs..

\(0.001567588\approx 0.001568\)

now put it in scientific notation

Answer 40

1.567588e-3

Answer 41

so 1.567*10^-3

Answer 42

ius it right

Answer 43

1.568*10^-3

Answer 44

you have to round up or down depending on the last number you're omitting, in this case that was a 7, so you round to the next number

Answer 45

ok

Answer 46

sorry it was a five, 0.001567\(\color{red}5\)88

so it's 1.568..

Answer 47

thanks

Answer 48

another question is 15.53 mL = 0.01553 L

right

Answer 49

yes that is correct

\[15.53 ml(\frac{1 L}{1000ml})=.01553 L\]