Question

1. What mass of C12H22O11 is present in the 25.0-mL diluted solution prepared in this experiment? Show your calculations.
2. How would the experimental (actual) molar concentration for C12H22O11 differ from the calculated concentration (higher, lower, or the same) given the following scenarios? Explain. (Hint: Compare the calculated concentrations to experimental concentrations).
3. A student spilled some of the solid C12H22O11 before adding it to the 50-mL volumetric flask.
4. A student added water so that is was about 5 mm higher than the indicated line on the volumetric flask.

c. When preparing the diluted solution, a student used the pipet bulb to blow out the last few drops in the pipet into the solution.

What volume of 0.08892 M HNO3 is required to react completely with 0.2352 g of potassium hydrogen phosphate?

HNO3(aq) + K2HPO4(aq) ⟶ H3PO4(aq) + KNO3(aq)

Image transcriptions

Report - Experiment 1 Preparation of Solutions DATA: Part 1 - Preparation of BaCO,(S) Molarity of BaCl2 solution Volume of BaCl2 solution 1.00m Back Mass BaCO;(s) + filter paper + evaporating dish 10.00 ml Backz 0.529 Mass filter paper + evaporating dish 48:715 L19. 2379 Mass of BaCO, (s) Part 2- Preparing a Mass Percent Stock Solution 2.3049 Calculated Mass of NaC 0.78/ 9 Calculated Mass of DI HO 419.2859 Experimental Mass of NaCl 0.78 1 9 Experimental Mass of DI H2O 49. 285 9 Color of Solution Part 3 - Preparing a Molarity Stock Solution Light pink Calculated Mass of C12H22011 Experimental Mass of C12H22011 2. 5679 2. 5 479 Color of Solution Part 4 - Preparing a Dilute Solution Dark Blue Volume of C12 22011 Stock Solution Used SML Total Volume of Dilute Solution 25 ML Color Difference between solutions in Parts 3 and 4 Light Blue Part 1 - Precipitation, Filtration, and Drying of Barium Carbonate 1. Using stoichiometry, calculate the mass of BaCO product, the theoretical yield for the reaction. Write the chemical equation first.