Question

To prepare a standard solution of Zn2+ you used a piece of metallic Zn, which was removed from54.2991 g piece to leave 53.3216 g. You place your sample of metallic Zn in a 500 mLvolumetric flask, add 20 mL of HNO3 and then dilute to volume. Next, you pipet a 1.00 mL ofthat solution into 150 mL volumetric flask and dilute to volume with water.A. What is the final concentration of Zn2+ in mg/L?Answer____________________Answer (practice exercise 4.2):B. What is the uncertainty of the Zn2+ concentration? Assume that the uncertainty in thebalance is \pm 0.1 and that you are using class A glassware.

          To prepare a standard solution of Zn2+ you used a piece of metallic Zn, which was removed from54.2991 g piece to leave 53.3216 g. You place your sample of metallic Zn in a 500 mLvolumetric flask, add 20 mL of HNO3 and then dilute to volume. Next, you pipet a 1.00 mL ofthat solution into 150 mL volumetric flask and dilute to volume with water.A. What is the final concentration of Zn2+ in mg/L?Answer____________________Answer (practice exercise 4.2):B. What is the uncertainty of the Zn2+ concentration? Assume that the uncertainty in thebalance is \pm 0.1  and that you are using class A glassware.

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