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Find the wt% KHP in an unknown via titration?

So in lab we had to find the wt% of KHP in an unknown (with another soluble salt). The wt% varies between 15-80%.

We used 0.1 M NaOH. 

I had 10.0216 g of unknown disolved in 250 mL of H2O. 

40 mL of the KHP solution took 29.90 mL NaOH and 29.85 mL NaOH to neutralize.

To find the wt%, this is my work

0.02990 L NaOH x 0.10mol/L NaOH = 0.002990 moles (of NaOH and KHP)

0.002990moles / 0.040 L = 0.07475m/L of KHP

0.07475moles x 204.218 g/mole = 15.265 g KHP / L

but because this was in 40 mL, I took 15.265 g x 0.04 = 0.610612 g/40 mL

and since it stared with 250 mL, I multiplied 0.6106 x (250/40) and got 3.81625 grams

3.816/10.0216 g  x  100 = 38.063 wt%

(and did the same for 29.85)

 

I'm just not sure if this is the correct way to do this. No one else that I've talked to has done it this way.

Any help would be appreciated!

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calculate the moles concept of the questions

1) 1 mole of sulphuric acid react with 1 mole of sodium carbonate to form salt, water and carbon dioxide.

write an equation?

 

ii) calculate the mass of the salt formedd when 10.6g of sodium carbonate are used in the reaction?

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Which of the following procedures would produce an effective pH=4.75 buffer? Briefly explain why or why not for each.

(a) Mix 50.0 mL of 0.10 M acetic acid with 50.0 mL of 0.10 M sodium acetate. 

(b) Mix 50.0 mL of 0.20 M acetic acid with 50.0 mL of 0.10 M sodium hydroxide.

(c) Start with 50.0 mL of 0.20 M acetic acid and slowly add sodium hydroxide until the pH reaches 4.75.

(d) Start with 50.0 mL of 0.20 M hydrchloric acid and slowly add sodium hydroxide solution until the pH reaches 4.75.

(e) Start with 50.0 mL of 0.20 M sodium acetate and slowly add hydrochloric acid solution until the pH reaches 4.75.

(f) Mix 50 mL of 0.10 mM acetic acid with 50.0 mL of 0.10 mM sodium acetate. 

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Okay, so the equation is as follows:

2KOH + K2Cr2O7 --> 2K2CrO4 + H2O

And my question is: 

Identify the oxidation numbers for each element in the equation. Then determine whether the equation describes a redox reaction. Justify your answer in terms of electron transfer. Describe the oxidation and reduction that occurs. 

I can figure out the oxidation numbers just fine. This is just confusing because I'm not sure if this is an acidic or basic solution, and I'm not sure how to describe the electron transfer in this equation. SOS!

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Ka NH4+ = 5.4 x 10-10.

Can you help? :/

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My apologies to my high school chemistry teacher but after 30 years I have forgotten just about everything you taught me....

The company that I work for manufactures a HHO generating hydrolysis system that when full has 3 gallons of 28% potassium hydroxide in water. Periodically it must be drained and flushed, at the time of the draining the volume of the system can be at any level from nearly zero to three gallons. I must create a chart showing how much 5% vinegar to add to the solution to bring the PH to a neutral point (~7) for disposal. The expected PH of the system when full is ~ 14.

The easiest method would be to simply bring the solution back to three gallons and neutralize at that point but it will often result in creating more volume than desired as I expect most systems to be somewhat less that full.

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Answer: Molarity of Acetic Acid in Vinegar = 0.175

 

I need to write discuss and explain my results for my university laboratory report. What are key points I can make?

 

Thanks in advance. 

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