3. 8.0 mL of HCIwas added into a10.0 mL graduatedcylinder andweighed on acentigram balance.Looking at thephoto to the right,record the mass tothe nearest 0.01Sost ha12.71graminyourdatatable (line 4)

When 8.0 mL of HCl was added to 10.0 mL graduated cylinder and weighted on a centigram balance. On…

Answered: 3. 8.0 mL of HC1 was added into a 10.0…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

< STARTING AMOUNT X A brine solution is 3.50% NaCl by mass. Given that its density is 1.071 g/mL , determine the quantity of liters of solution that contains 5.00 moles of NaCl 5.00 ADD FACTOR 0.1 *( ) 3.50 10 35.45 Question 29 of 33 1.071 0.01 8.03 x 1022 1000 100 ANSWER 7.80 22.99 0.0156 L solution g NaCl/mL g solution mL solution kg solution g NaCl/g solution 58.44 6.022 x 1023 0.0780 moles of NaCl mol NaCl RESET 0.001 2 1 g NaCl 1.56
2.93 g Measured Volume of Water: 100.0 mL each question with correct significant figures and units. You must show calculations for determining each quantity. If necessary, use the molar mass of NaCI = 58.44 g/mol. You will be asked to show your work for each question. A.Determine the number of moles of NaCI in the solution B.Determine the number of moles of all solutes (both cations and anions) from the number of moles of NaCI that you determined above. C. Determine the mass (in kg) of solvent (assume that the density of water is 1.000 g/mL). D. the molality of all solutes.
Percent by Mass= Mass of Solute x100 Percent by volume and Percent by Mass calculations Mass of Solution Volume of Solute Name: Percent by Volume= -x100 Volume of Solution 1. 1. Calculate the percent by volume if 56.7 ml of alcohol is added to 540 ml of water. (Remember to add both solute and solvent to get the total volume of solution to put on the bottom.) 540 15.23 2 Calculate the percent by mass if 35.0 grams of NaC! is added to 455 grams of water to make a salt solution. 3. Calculate the percent by volume if 15.5 ml of HCI is added to 1.0 Liter of water. 4. Calculate the amount of water needed to make a 5% solution of alcohol, if you have 25 ml of alcohol? (Hint: first you will need to find the total amount of solution needed. then subtract the 25 ml from that.)
Jacquel Adding or subtracting and multiplying or dividing measurements A chemistry student must write down in her lab notebook the concentration of a solution of potassium chloride. The concentration of a solution equals the mass of what's dissolved divided by the total volume of the solution. Here's how the student prepared the solution: • The label on the graduated cylinder says: empty weight: 4.200 g • She put some solid potassium chloride into the graduated cylinder and weighed it. With the potassium chloride added, the cylinder weighed 71.0 g. • She added water to the graduated cylinder and dissolved the potassium chloride completely. Then she read the total volume of the solution from the markings on the graduated cylinder. The total volume of the solution was 133.0 mL. What concentration should the student write down in her lab notebook? Be sure your answer has the correct number of significant digits. Ch 8 mL Explanation Check O2021 McGraw-Hill Education All Rights Reserved…
Calculate the molarity of each solution. 42.2 mg of KI in 118 mL of solution Express your answer using three significant figures.
A particular brand of beef jerky contains 6.05x10-2% sodium nitrite by mass and is sold in an 8.00-oz bag. Y Part A What mass of sodium does the sodium nitrite contribute to sodium content of the bag of beef jerky? Express your answer to three significant figures and include the appropriate units.
One half tsp of table salt (NaCl) weighs aproximately 2.0 grams. (You will need to look up the molar mass for NaCl) There are approximately 237 ml in a cup. Determine the Molarity of the solution 1 cup water with one half tsp table salt. Determine the molarity of this solution using the formula M=g/MM/L. What is the molarity? Show your calculations. (Remember to convert 237 mL to L)
If you titrate 25.00 ml of a 410. mg/L ascorbic acid solution and titrate it with 1.38x10 M KIO, what volume of titrant (ml) will you use? Please ensure that you include units (ml). Please report your answer to the correct number of significant figures. Answer: If you titrate 25.00 ml of a 480. mg/t ascorbic acid solution, boil it for 15 minutes and then titrate it with 125 mt of 1.34x10 M KIO, What is the concentration of Vitamin C in mg/g ascorbic acid ( original) (mg/9? Answer: And finally, If you boil 26.97 g of juice and then titrate it with 10.55 ml. of 1.16x10 M KIO, what is the concentration of vitamin C in mg per gram of juice (mg/g)? Piease remember to include units (mg/g) of Please remember to use the correct number of significant figures. tion Answer:
One of the Ionic compounds in sports drinks is potassium di hydrogen phosphate. The label on one of these sports drinks tells us that 240 mL of the solution contains 30 mg of potassium. KH2PO4 is the only ingredient that can provide potassium. how many grams of KH2PO4 are dissolved in 240 mL of the solution? What is the molars ty of KH2PO4 in this solution? Organize abs label your calculations so that they are presented in a logical manner for full credit
A chemist prepares a solution of calcium bromide (CaBr,) by measuring out 68. g of calcium bromide into a 450. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's calcium bromide solution. Round your answer to 2 significant digits. mol/L x10
or dividing measurements A chemistry student must write down in her lab notebook the concentration of a solution of sodium hydroxide. The concentration of a solution equals the mass of what's dissolved divided by the total volume of the solution. Here's how the student prepared the solution: • The label on the graduated cylinder says: empty weight: 5.250 g • She put some solid sodium hydroxide into the graduated cylinder and weighed it. With the sodium hydroxide added, the cylinder weighed 75.41 g. • She added water to the graduated cylinder and dissolved the sodium hydroxide completely. Then she read the total volume of the solution from the markings on the graduated cylinder. The total volume of the solution was 37.4 mL. What concentration should the student write down in her lab notebook? Be sure your answer has the correct number of significant digits. -1 Explanation Check 2021 McGraw-Hill Education All Rights Reserved Terms of Use Privacy Accessibility Thank The # $ % & 2 3
For the following questions (1-5), consider the compound tartrazine (Yellow 5 food dye) that has a chemical formula of C16H9N4Na3O9S2. Ana weighs out 0.1328 g of tartrazine powder on the balance for her experiment and makes a stock solution by dissolving her powder in 500.0 mL of solution. 1. Determine the number of moles of tartrazine that Ana weighed out. 2. Find the molarity (mol/L) of Ana’s tartrazine solution. 3. Ana makes 5 tartrazine standards by diluting her solution and measures their absorbances using a spectrophotometer: 4. Calculate the molar extinction coefficient (molar absorptivity) of tartrazine in units of 1/(M·cm). Assume a cuvette path length of 1.00 cm. 5. If Ana determines the absorbance of an unknown tartrazine sample to be 0.662, what is the concentration of the sample in µM?

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS

3. 8.0 mL of HC1 was added into a 10.0 mL graduated cylinder and weighed on a centigram balance. Looking at the photo to the right, record the mass to the nearest 0.01 gram in your data table (line 4) SoNt ha 12.71