Chapter 1, Problem 2P

$ F4 An aqueous solution of 2.87 M hydrochloric acid, HCl, has a density of 1.05 g/mL. The percent by mass of HCl in the solution is %. Submit Answer % 5 T G F5 Retry Entire Group 9 more group attempts remaining 6 Cengage Learning | Cengage Technical Support Y H [Review Topics] [References] Use the References to access important values if needed for this question. MacBook Air F6 & 7 gilinent-take F7 8 00 1 DII FB K ( 9 F9 0 L ) O A F10 P Chapter Previous + 11 X Next ☐ Save and Exit OWLY S deles

Drug Stock solution concentration = 10 millimolars Desired drug solution concentration = 10 micromolars The final solution will be inserted into a well that can hold 8 to 10 mL of solution. How much stock solution and solvent must be used to change the 10 millimolars stock solution to 10 micromolars?

Jollibee Burger     Item                             Sodium(mg)                Fat(g)              Calories           Item cost($) Beef Patty                               50                                17                   220                  $0.25 Bun                                         330                             9                      260                  $0.15 Cheese                                     310                              6                     70                   $0.10 Onions                                     1                                  2                     10                    $0.09 Pickles                                     260                              0                      ,. 5                   $0.03 Lettuce                                    3                                  0                      4                      $0.04 Ketchup                                   160                              0                      20…

1. (answer the questions in the tan boxes in the tables below each question) A student conducted an investigation to determine the effect of water temperature on the amount of sugar that dissolves in a beaker of water. Identify components for trial 1 of this investigation. Beaker Number 1 2 3 4 Amount of Water (mL) 100 100 100 100 Amount of Water (mL) Trial 1 Temperature of Temperature of Amount of Sugar Sugar (°C) Water (°C) Dissolved (g) 20 20 20 20 Temperature of Sugar 5 10 15 20 185 189 194 204 Temperature of Water Terms Variable Constant Amount of Sugar Dissolved

For questions #14-16, you should do your work on a separate piece of paper and then upload it. You should use the GUESS Method of solving for each problem. Also, you have a choice. You can complete both #14 & #15 which are single step question or do the extension problem which is a 2 step problem instead of 14 & 15. You must complete #16. Equations Q = mcAT Q = ±mLf Q = ±mLv Values for Water Clice) = 2.06 J/g°C C(water) = 4.186 J/g°C C(steam) = 1.87 J/g°C Lf (water) = 333 J/g Lv (water) = 2,260 J/g %3D G- S- U- E- S- #14. Calculate the energy required to heat 12.5 g of water from a temperature of 42.2°C to 52.3°C. #15. How much thermal energy is needed in order to turn 15.7 grams of water into ice? Extension: We start with 23.2 grams of ice at 0°C and add heat to the ice. The ice completely melts and then is heated until it reaches 45.3°C. How much energy is added in total? #16. 12.0 g of a metal absorbs 317 J when it is heated from 38.2°C to 82.7°C. What is the specific heat of the…

What is the difference between a decigram balance and an analytical balance?

A 106.2 mL sample of 0.100 M methylamine ( CH3NH2; Kb = 3.7 x 10-4) is titrated with 0.235 M HNO3. Calculate the pH after the addition of each of the following volumes of acid.

Solution 1 is diluted by combining 6 mL of Solution 1 with 64 mL of Solution 2. What is the dilution of solution 1?   Report your answer in standard decimal notation rounded to two decimal places. For example, 4 mL added to 16 mL would be a 0.20 dilution. Include trailing zeros if necessary so your answer has two decimal places.

It is always important to label everything in the dispensary or the medicinal chemistry laboratory. One student made aspirin and the other student made paracetamol. Both students left their unlabelled samples near the balance. Give details of two techniques that you could use to distinguish between these samples