I want to prepare 100.00 mL of a ≈0.1000 M KNO3 solution (FW = 101.1032 ± 0.0008 g mol-1). I weigh out 2.1525 g of KNO3 and dissolve in 100 mL. What is the molar concentration with absolute/relative uncertainty? • the balance has an uncertainty of ± 0.0002 g • the volume has an uncertainty of ±0.08 mL
I want to prepare 100.00 mL of a ≈0.1000 M KNO3 solution (FW = 101.1032 ±...
n titration of 50.00(±0.01) mL an acetic acid solution with a 0.1000 (±0.0004) molar NaOH solution (as the titrant), the initial and final (end point) buret readings are as follows: Initial buret reading: 0.07 (±0.01) mL Final buret reading: 5.72 (±0.01) mL Calculate the concentration of acetic acid and the percent relative uncertainty related to it. Report ONLY the percent relative uncertainty in the provided box with correct number of significant figures.
The final volume of buffer solution must be 100.00 mL and the final concentration of the weak acid must be 0.100 M. Based on this information, what mass of solid conjugate base should the student weigh out to make the buffer solution with a pH of 5.00? MISS Based on this information, what volume of acid should the student measure to make the buffer solution? volume =
A 48.8-mL sample of a 7.8 M KNO3 solution is diluted to 1.20 L . 1.What volume of the diluted solution contains 10.0 g of KNO3? (Hint: Figure out the concentration of the diluted solution first.)Express your answer using two significant figures. 2. To what volume should you dilute 130 mL of an 8.00 M CuCl2 solution so that 50.0 mL of the diluted solution contains 5.7 g CuCl2? Express your answer using two significant figures.
.A 7.88% (w/w) Fe(NO.). (fw = 241.86 ) solution has a density of 1.062 g/mL. Calculate (a) the molar analytical concentration of Fe(NO3)3 - (b) the molar NO concentration. (c) the grams of Fe(NO): contained in each liter.
A solution of F− is prepared by dissolving 0.0887±0.0006 g NaF (molar mass = 41.989±0.001 g/mol) in 152.00±0.09 mL of water. Calculate the concentration of F− in solution and its absolute uncertainty.
I have a 0.125 M sodium oxide solution a) 15.25 mL of this is diluted to 100.00 mL total volume. What is the concentration of the new solution? b) I now want to make 75.00 mL of a 20.00 mM solution. What volume of the 0.125 M solution must be diluted to 75.00 mL to make this? c) What is the concentration of sodium ions in the 0.125 M sodium oxide solution?
A solution of HNO is standardized by reaction with pure sodium carbonate 2H+ + Na,CO3-2 Na+ + H2O + CO2 A volume of 25.29 + 0.05 mL of HNO3 solution was required for complete reaction with 0.8380+0.0008 g of Na,CO3. (FN 105.988 0.001 g/mol). Find the molarity of the HNO3 solution and its absolute uncertainty. Note: Significant figures are graded for this problem. To avoid rounding errors, do not round your answers until the very end of your calculations IHNO,I-I...
A 50:8-mL sample of a 5.4 M KNO3 solution is diluted to 1.20 L. Review Part A What volume of the diluted solution contains 12.0 g of KNO,? (Hint: Figure out the concentration of the diluted solution first.) Express your answer using two significant figures. να ΑΣφ L Request Answer Submit <Return to Assignment Provide Feedback
I MAINLY NEED HELP ON TABLES PLS HELP THANK YOU Materials: NaOH MW = 40 g/mL, KHP - potassium hydrogen phthalate, KHC2H4O4, MW = 204.23 g/mol. Acetic acid, HC2H302, MW = 60.05 g/mol Part 1: Standardization of NaOH Assume 0.951 g of KHP is weighed and transferred to a 250 mL Erlenmeyer flask. Approximately 50 mL water is added to dissolve the KHP. Note that the exact volume of water is not important because you only need to know the...
References Mailings Review View 1) A bottle on the shelf is labeled 0.125 M HNO, (HNO, has a molar mass of 63.02 g/mol) (a) of measure out 30.0 mL of that solution, what mass of HNO, does it contain? (b) What volume of that solution should I measure if I have a reaction that requires 0.0620 mol of HNO3? 2) If I dissolve 10.0g of sodium phosphate, Na PO: (molar mass 163.95 g/mol), in a total volume of 500.0 mL...