It is often necessary to do calculations using scientific notation when working chemistry problems. For practice, perform each of the following calculations. 1.00 x 10-8 +1.54 x 10-4 2.68 x 104 +9.67 × 105 5.49 × 104 = 6.40 x 10-5 (1.00 × 10-8) (1.54 × 10-4) Submit Answer Retry Entire Group 9 more group attempts remaining

Using the calibration curve below (equation of the line: y=0.0039x + 0.9981) to determine the percentage of sugar in a sugar water solution with a density of 1.034 g/mL. Density versus Percent Sugar 1.07 1.06 y = 0.0039x + 0.9981 R² = 0.9998 1.05 1.04 1.03 1.02 1.01 1 0.99 6 8 10 12 14 16 Percent Sugar (% m/m ) 8.5% 1.0% 9.2% 4.2 % 9.9% Density (g/mL) 2.

A student sets up the following equation to solve a problem in solution stoichiometry. (The ? stands for a number the student is going to calculate.) Enter the units of the student's answer.   I'm confused on what the next step is from here. I dont know if I need to switch the 10-3 to the bottom to make the 103 and how would I solve the problem from here?

To prepare a solution of KCl, you weigh out 1.5672 (± 0.0003) g and dissolve it in a volumetric flask of 250.00 (±0.50) mL in volume. Express the molarity of the solution and its uncertainty with appropriate number of significant figures. (Formula mass of KCl is 74.551 ± 0.004 g/mol)

The following volumes of 0.000300 M SCN are diluted to 15.00 mL. Determine the concentration of SCN in each sample after dilution. These values will be used during the experiment. To enter exponential values, use the format 1.0e-5. Sample 0.000300 M SCN (mL) [SCN'] (M) 1 1.50 3.50 7.00 4 10.00 3.

Please use the corrrect significant digits (3), if needed use scientific notation.

please answer this is dimensional analysis as the problem requires

You are in the lab preparing copper solutions for the MICRO lab this week. You measure 0.1035 (±0.0001) g of copper metal and dissolve it in a few mLs of concentrated nitric acid. This solution is diluted to the mark with water in a 50.00 (±0.05) mL volumetric flask. You withdraw a 5.00 (±0.01) mL aliquot with a volumetric pipet and deliver it to a 100.00 (±0.08) mL volumetric flask. After dilution to the mark with water, calculate the concentration and the absolute error in a solution of copper in ppm (assume ppm = 1 µg/g = 1 µg/mL = 1 mg/L).

4:31 PM Time's Up! What is the mass in grams of KBr in 0.400 STARTING AMOUNT X ADD FACTOR 8.43 x 10²² 0.350 39.10 g KBr 3 9.60 x 10-³ 0.140 mol KBr 5.47 7.09 x 102⁰ 1 L L of a 0.350 ANSWER M KBr 0.400 136 M solution? RESET 5 16.7 1.18 x 10-³ g KBr/mol 6.022 X 119 mL

Compute (4.29 x 105) · (1.89×10-4). Express your answer to three digits.