- What mass of C12H22O11 is present in the 25.0-mL diluted solution prepared in this experiment? Show your calculations.
- 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).
- A student spilled some of the solid C12H22O11 before adding it to the 50-mL volumetric flask.
- 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)
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.
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