Without using a calculator, decide which would give a significantly smaller value than 6.12 × 10-2, which would give a significantly larger value, or which would give essentially the same value. 6.12 x 10-2 +1.10 × 10 6.12 × 10-2 – 1.10 × 105 6.12 × 10-2 x 1.10 × 10 6.12 × 10-2 ÷1.10 × 105

Without using a calculator, decide which would give a significantly smaller value than 6.12 × 10-2, which would give a significantly larger value, or which would give essentially the same value. 6.12 x 10-2 +1.10 × 10 6.12 × 10-2 – 1.10 × 105 6.12 × 10-2 x 1.10 × 10 6.12 × 10-2 ÷1.10 × 105

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter14: Mixtures And Solutions

Section: Chapter Questions

Problem 1STP

See similar textbooks

Similar questions

How many significant figures is present in the following measurement? volume of 0.1004 M BaCl2 titrant added = 12.67 mL
Determine the amount of potassium chloride in each solution. 18.9 g of a solution containing 1.12 % KCl by mass Express your answer in grams using three significant figures. 29.2 kg of a solution containing 20.7 % KCl by mass Express your answer in kilograms using three significant figures. 45 mg of a solution containing 14 % KCl by mass Express your answer in milligrams using two significant figures.
A chemist prepares a solution of zinc oxalate (ZnC2O4 )by measuring out 4.97 mg of zinc oxalate into a 300. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in /molL of the chemist's zinc oxalate solution. Round your answer to 3 significant digits.
Chemistry An analytical chemist weighs out 0.410g of an unknown triprotic acid into a 250mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.0700M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 91.5mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits.
A chemist prepares a solution of copper(II) fluoride (CuF2) by measuring out 0.058g of copper(II) fluoride into a 300.mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in /molL of the chemist's copper(II) fluoride solution. Round your answer to 2 significant digits.
The concentration of PSA (prostate-specific antigen) in the blood is sometimes used as a screening test for possible prostate cancer in men. The value is normally reported as the number of nanograms of PSA per milliliter of blood. A PSA concentration of 1.7 ng/mL1.7 ng/mL is considered low. Express that value in terms of the units shown. PSA= g/L PSA= kg/m3 PSA= mg/L
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?
You perform your first titration using your NaOH with a KHP solution. Your KHP solution is made with 0.5045 g of KHP. The initial amount of NaOH in your pipette is 16.26 mL and the final amount in your buret is 36.79 mL when the indicator changes colour. Determine the concentration of your NaOH solution. Write your answer to four decimal places without units.
Part 1 – Preparation of CaCO3(s) The following is a procedure that was theoretically performed by a student. Read through the procedure and answer the questions below. A 10.0 mL graduated cylinder to measure 10.0 mL of a 1.00 M CaCl2 solution into an initially empty 50.0 mL beaker. A 50.0 mL graduated cylinder was then used to measure out 25.0 mL of 0.500 M K2CO3. This K2CO3 solution was then added to the beaker containing the CaCl2 The solution became cloudy, and the student concluded that a precipitate must have formed. Write a balanced chemical reaction below, including phases, and identify the chemical formula of the precipitate: Answer the questions below as part of Data Analysis. 1. What is the actual yield of the product? 2. Using stoichiometry, calculate the limiting reactant, and the theoretical yield (the mass of CaCO3 product) for the reaction. 3. Determine the percent yield of the reaction.
Solution 0.549*10^-82 is wrong, 0.1098x10^-80 is also wrong. This question is not graded.
please see image attached: A chemistry student weighs out 0.146 g of chloroacetic acid into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1400M(molarity) NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the equivalence point. Round your answer to 3 significant digits.
0.50 M NaOH used. I need to calculate these 3 things based off the results from attached "Data table 1": 1). Average Volume of NaOH used (mL) 2). Concentration CH3COOH in vinegar (mol/L) 3). % CH3COOH in vinegar