The pH of a solution is 5.84 ± 0.05. What is the concentration of H+ in the solution and its absolute uncertainty? -6 [H*] = 1.45 x10 1.67 x10-7 M M Incorrect

Lab 7

Make sure answer has correct significant digits

Students performed three KHP titrations in Part 1 to standardize their NaOH solution. They reported the following measurements:   Determination #1 Determination #2 Determination #3 Mass of KHP + Vial 14.0862 g 14.5621 g 14.3998 g Mass of 'Empty' Vial 13.2492 g 13.7695 g 13.6887 g Final Burette Reading 45.10 mL 38.53 mL 37.17 mL Initial Burette Reading 5.08 mL 0.52 mL 3.19 mL How many moles of NaOH did they use in their first titration? Report your answer to the correct number of significant figures

Which of the options is the right answer ?

1-13. Why is it more accurate to say that the concentration of a solution of acetic acid is 0.01 F rather than 0.01 M? (Despite this distinction, we will usually write 0.01 M.) 1 /T M fN- CL han 20 0

A sample contained a mixture of NaHCO3, NACO, and inert material. If A represents the millilitres (mL) of standard acid to reach the phenolphthalein end point and B the volume of acid needed to go from this point to the methyl orange end point, which of the following relationships will be obserrved? O A B>A, A>0 O B. A>B; B>0 OC A=0, B>A O D. None of the given answers OE. A-B, B>0

Answer both parts please

how do i find the absolute and relative uncertainty of my data?

Ben ran through the experiment and found the best-fit line listed below for his standard calibration curve of absorbance vs concentration in M. y = 3214.0x + 0.0076   Ben then prepared a solution that had 5.00 mL 0.002 M iron(III) nitrate in 1 M nitric acid, 3.00 mL 0.002 M potassium thiocyanate, and 2.00 mL DI water. If the absorbance for the solution was 0.436, calculate the equilibrium concentration of iron(III) thiocyanate in the solution. Report your answer in mM with three places after the decimal.