@ In my aby I used a technique to measure H concentration. If I measure the...
Question 11 You use an analytical balance to measure the mass of a weigh boat and record a mass of 1.5624 g. You then add some NaHCO, to Not changed since the weigh boat and give the welgh boat to your lab partner to measure. Your lab partner mistakenly forgets to record all of the digits on the balance and records a mass of 1.92 g What is the minimum number of grams of acetic acid that you would need...
1.
2. for this problem for my Ka on acid 1 I got :
4.3651583224 x 10^-6 . for my acid 2 i got :
2.5118864315 x 10^-2. and for my acid 3 I got:
3.7239170625 x 10^-6. What is the correct number
of sig figs?
solution initial components change initial type (check all that apply) acidic effect of change on pH (check one) O pH higher O pH lower O pH the same 4,0 basic add Nal neutral acidic...
Hello! I was wondering if anyone can check my work on my prelab
calculation as I feel iffy about it. the question asks "calculate
the mass of H2C2O4•2H2O you will require to react with about 16 ml
of your potassium permangate solution". So I used the moles of our
solution which was 0.02 as a conversion factor to get to the grams
of H2C2O4, is this correct
or did I do something wrong?
1122 4 + 2 KMnO4 8 CO₂...
A student plans to measure the concentration of a basic sample by titration with HCℓ. In order to standardize the HCℓ, a primary standard solution is made by weighing 0.7235 g of "tris" base (H2NC(CH2OH)3 - it is monobasic), quantitatively transferring the powder to a 500 mL volumetric flask, and diluting to volume with deionized water. A 10.00 mL aliquot of the tris solution is taken for titration. What is the concentration of tris in the primary standard, in M?...
pH is a logarithmic scale used to indicate the hydrogen ion concentration, [H+], of a solution: pH=−log[H+] Due to the autoionization of water, in any aqueous solution, the hydrogen ion concentration and the hydroxide ion concentration, [OH−], are related to each other by the Kw of water: Kw=[H+][OH−]=1.00×10−14 where 1.00×10−14 is the value at approximately 297 K. Based on this relation, the pH and pOH are also related to each other as 14.00=pH+pOH Part B Part complete 0.25 g of...
pH is a logarithmic scale used to indicate the hydrogen ion concentration, [H+], of a solution: pH = -log[H+]Due to the autoionization of water, in any aqueous solution, the hydrogen ion concentration and the hydroxide ion concentration, [OH-], are related to each other by the Kw of water: Kw = [H+][OH-] = 1.00 x 10-14where 1.00 x 10-14 is the value at approximately 297 K. Based on this relation, the pH and pOH are also related to each other as 14.00 = pH...
i need help with these three questions
Incorrect Question 2 0/1.25 pts 0.678 g of KHP is used to standardize a NaOH solution. If it took 31.55 mL of NaOH to neutralize the KHP, what is the concentration of the NaOH solution? The molar mass of KHP is 204.22 g/mol. KHP + NaOH --> NaKP + H2O Give the answer to 3 sig figs and use units of M 0.0214 Unanswered Question 3 0/1.25 pts A 25.00 mL HCl sample...
how would I calculate my results from the first two data the
first data is my results and the second data I have to calculate
each of those with the information that I have on the first 3
trails I really really need help and i just dont understand thank
you.
1 concentration of EDTA solution 2 molar mass of CaCO3 0.0100 M 100.09 g/mol Trail 1 -Trail 2 Trail 3 12 12.01 11.99 5 Unknown analysis Part 1 (pH...
What is the concentration of the H(2)SO(4) solution?
Exactly 34.4 mL of 0.1013M KOH was used to titrate a 25.0 mL sample of H2SO4. What is the concentration of the H2SO4 solution? O 0.234 M O 0.118 M O 0.140 M 0.0697 M. O 0.278 M
I am needing help to solve this table. specifically the step 4
portion. My 2 compounds that I'm using for this experiment are 0.1
M NaHCO3 (acid) and 0.1 M Na2CO3. im having issues finding the
concentration and pKa of everything.
thank you!
Step 1 hydrogen carbonate/carbonate (HCO3/003-) [NaHCO₃ and Nagco ₂] Initial Buffer: Pour 10 mL of the acid component of your buffer into a 50-ml beaker. Add 10 mL of the conjugate base of your buffer, and mix....