Bar-code scanners at supermarkets emit orange-red laser light with a wavelength of 633 nm. If the energy output of these scanners is 1.0 mJ per second, how many photons are released if the scanner operates for 2.0 seconds? otassiur metal

Bar-code scanners at supermarkets emit orange-red laser light with a wavelength of 633 nm. If the energy output of these scanners is 1.0 mJ per second, how many photons are released if the scanner operates for 2.0 seconds? otassiur metal

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.102QE

See similar textbooks

Similar questions

Follow the directions of Question 64. Consider two beakers: Beaker A has a weak acid(K a=1105). Beaker B has HCI. The volume and molarity of each acid in the beakers are the same. Both acids are to be titrated with a 0.1 M solution of NaOH. (a) Before titration starts (at zero time), the pH of the solution in Beaker A is the pH of the solution in Beaker B. (b) At half-neutralization (halfway to the equivalence point), the pH of the solution in Beaker A the pH of the solution in Beaker B. (c) When each solution has reached its equivalence point, the pH of the solution in Beaker A the pH of the solution in Beaker B. (d) At the equivalence point, the volume of NaOH used to titrate HCI in Beaker B the volume of NaOH used to titrate the weak acid in Beaker A.
A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
A monoprotic organic acid that has a molar mass of 176.1 g/mol is synthesized. Unfortunately, the acid produced is not completely pure. In addition, it is not soluble in water. A chemist weighs a 1.8451-g sample of the impure acid and adds it to 100.0 mL of 0.1050 M NaOH. The acid is soluble in the NaOH solution and reacts to consume most of the NaOH. The amount of excess NaOH is determined by titration: It takes 3.28 mL of 0.0970 M HCl to neutralize the excess NaOH. What is the purity of the original acid, in percent?
Consider 1.0 L of an aqueous solution that contains 0.10 M sulfuric acid to which 0.30 mole of barium nitrate is added. Assuming no change in volume of the solution, determine the pH, the concentration of barium ions in the final solution, and the mass of solid formed.
For the determination of basic species in 0.1878 g Talcid sample; 20 mL of 0.1009 M HCl solution was added to the sample and the necessary procedures were carried out and titrated with 0.1097 M NaOH solution. Since 10.2 mL of base solution is consumed at the end of the titration, which of the following is the% base amount in CaCO3? (CaCO3: 100,087 g / mol) A. 23.96B. 55.1C. 45.1D. 42.1
Consider the titration of 100.0 mL of an unknown concentration of weak monoprotic acid with 0.550 M NaOH. If 25.00 mL is required to reach the end-point, what is the concentration of the weak acid? Answer in units of moles per litre.
A student is conducting a titration between a weak, monoprotic acid and sodium hyhroxide, NaOH. The student needs to make 250. mL of 0.150 M weak acid from a 4.00 M stock solution. a. Determine the volume, in mL, of 4.00 M stock solution the student needs to prepare 250. mL of 0.150 M weak acid. b. Describe the procedure the student should use to make 250.0 mL of 0.150 M weak acid using appropriate equipment selected from the list below. - 250 mL beaker, 250 mL graduated cylinder, 250 mL volumetric flask, 50 mL Buret filled with 4.00 M weak acid, 500 mL wash bottle filled with distilled water. c. The student titrates 20.0 mL of the weak acid with 0.300 M sodium hydroxide, NaOH (aq). When 5.00 mL of NaOH (aq) has been delivered the pH of the weak acid is 5.328. i. Determine the concentration of H3O+1. ii. Determine the Ka of the weak acid. d. The student continues to titrate the weak acid to equivalence. i. What volume of NaOH (aq) is required to…
A titration of 25.00 mL of an unknown HCl solution with 0.1550 M NaOH starts at a buret reading of NaOH of 0.33 mL. The phenolphthalein indicator turns light pink in the acid solution over 30 seconds at a buret reading of 24.19 mL. Write the balanced equation for the neutralization reaction. What is the molarity of the HCl solution?
A 0.2071-g sample of an unknown monoprotic acid is dissolved in water and titrated with standardized potassium hydroxide. The equivalence point in the titration is reached after the addition of 33.06 mL of 6.814×10-2 M potassium hydroxide to the sample of the unknown acid. Calculate the molar mass of the acid. B. Calculate the volume of 0.212 M barium hydroxide required to neutralize 27.0 mL of a 0.198 M perchloric acid solution. C. Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory as a primary standard. It has the unwieldy formula of KHC8H4O4. This is often written in shorthand notation as KHP.If 26.28 mL of a potassium hydroxide solution are needed to neutralize 2.025 grams of KHP, what is the concentration (mol/L) of the potassium hydroxide solution?
A 44.6 mL of 0.103 M HCI is added to an antacid sample. The solution is titrated to a bromophenol blue endpoint using 19.8 mL of 0.0998M NaOH. How many moles and how many grams of the base are in the antacid sample? Assume the active ingredient is MgCO3. Moles of NaOH? Moles of HCl? Moles of MgCO3? Mass of MgCO3?
In this assignment, you will determine the mass % of an unknown sample of baking soda (NaHCO3) by titrating it with an HCl solution of known concentration. The laboratory will open with a beaker on the stir plate with 1.5000 g of impure solid NaHCO3 and with sufficient water added to make the total volume 25.00 mL. The buret will be filled with 0.3015 M HCl. Pouring HCI until pH is 2. The volume in the buret went from 0 mL to 43 mL Question 1: Calculate the moles of HCl transferred during the titration. (number and unit) (Keep four significant digits in all of the calculations.) Question 2: How many moles of NaHCO3 are present in the sample? Question 3: What mass of NaHCO3 is present in the sample? Question 4: What percent of the original sample mass was NaHCO3?
A weak acid- strong base titration was performed as follows: 10.00 mL of 0.10 M acetic acid were collected in an Erlenmeyer flask, and then diluted to 100 mL with distilled water. After that, two drops of indicator were added. Then, the buret was filled with 0.100 M NaOH. The titration was started by slowly adding NaOH to acetic acid. (Note: The volume of two drops indicator is ignored as it is so tiny compared with 100 mL.) What is the pH of the solution in the Erlenmeyer flask after adding 10.00 ml of 0.100M NaOH? Select one:a. 8.35b. 6.9c. 7.22d. 7.00