A student would like to prepare a 0.010 M solution from a 1.0 M stock solution with minimal error. The student can choose to do a one-step dilution that uses a 10 mL transfer pipet and a 1000 mL volumetric flask or a two-step dilution using a 50 mL pipet and a 1000 mL volumetric flask for the first dilution, and a 100 mL pipet and a 500 mL volumetric flask for the second dilution. Which method has the smallest overall relative uncertainty and what is the value? **Use table 4.2 on page 70 in your textbook for tolerances of the glassware. O One-step dilution; 0.0020 Two-step dilution; 0.0020 O Two-step dilution; 0.0014 O One-step dilution; 0.0010

4) did i do this right?

A student needs to measure out ~17mL of a solution to add to a reaction container, select all pieces of equipment that can be used to accomplish this task: Group of answer choices a 20-mL beaker a 50-mL beaker a 25-mL Erlenmeyer flask a 10-mL graduated cylinder a 25-mL graduated cylinder a volumetric flask a volumetric pipet

5.00 mL of stock solution is diluted to 25.00 mL, producing solution ALPHA. 10.00 mL of solution ALPHA is diluted to 25.00 mL, resulting in solution BETA. 10.00 mL of solution BETA is then diluted to 25.00 mL, producing solution GAMMA. dilution factor for ALPHA from stock solution = 0.167 dilution factor for BETA from ALPHA solution = 0.0476 part c and d?

If you wanted to create a 2 mM solution of sodium chloride in 1000 mL from a 200 mM sodium chloride stock solution, what volume of the solution would you use? (hint: M1V1 = M2V2).

Make sure answer has correct significant digits

||| Microsoft O W OCHEMICAL REACTIONS Dilution A chemist must prepare 500. mL of 1.00 M aqueous silver perchlorate (AgCIO4) working solution. She'll do this by pouring out some 1.94 silver perchlorate stock solution into a graduated cylinder and diluting it with distilled water. Calculate the volume in mL of the silver perchlorate stock solution that the chemist should pour out. Be sure your answer has the correct number of significant digits. 00 mL Microsoft Microsoft 6.52.210... Explanation Check 9,180 ☐ X 285 S C Q NOV 10 ||| tv SO17 A mol L ( aqueous 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility P eBook W 1 0

A chemistry student is given 1.00 L of a clear aqueous solution at 17 degrees Celsius. He is told an unknown amount of a certain compound X is dissolved in the solution. The student allows the solution to cool to 17 degrees Celsius. The solution remains clear. He then evaporates all of the water under vacuum. A precipitate remains. The student washes, dries and weighs the precipitate. It weighs 0.12 kg. Using only the information above, can you calculate the solubility of X in water at 17° C? If you said yes, calculate it and be sure your answer has a unit symbol and 2 significant digits.

OCHEMICAL REACTIONS Dilution A chemist must prepare 875. ml. of 335. M aqueous copper (11) fluoride (CuF) working solution. She'll do this by pouring out some 407. µμM aqueous copper (11) fluoride stock solution into a graduated cylinder and diluting it with distilled water. Calculate the volume in ml. of the copper (11) fluoride stock solution that the chemist should pour out. Round your answer to 3 significant digits. 0 04 0/5 Y

You measure 15.0 mL of the H2C2O4 solution with a 100-mL graduated cylinder and add it to a 125-mL Erlenmeyer flask.  Then you add two drops of the indicator, phenolphthalein, to the oxalic acid solution in the flask.  You dispense the NaOH solution from the buret into the flask (while swirling the flask) until you reach the endpoint.  At the endpoint, the solution in the flask turns light pink.  You repeat the titration two additional times for a total of three trials.  H2C2O4 (aq) + 2 NaOH (aq) --> Na2C2O4 (aq) + 2 H2O (l)                                                (I)              (II)                (III) Volume of H2C2O4 used  15.00 mL   15.00 mL   15.00 mL how many Moles H2C2O4 are used in each trial?