CIVIL 4210 Spring 23 exams

When 100. mL of 1.0 M HCl is added to a 2.0 g piece of CACO3, CO2 is produced at a certain rate. Which of the changes below will NOT increase the rate of this reaction? a. Adding 100, mL of 2.0 M HCl in place of 100. mL of 1.0 M HCI. b. Heating the 100. mL of 1.0 M HCl before adding it to the СаСОз. c. Adding 100. mL of 1.0 M HCl to 2.0 g of powdered CaCO3. d. Adding 150. mL of 1.0 M HCl in place of 100. mL of 1.0 M HCI.

Help with 18 please.

A 500 mL sample of waste water contains 42.65 ug of mercury, Hg. If the density of the sample is 1.073 g/mL. Calculate the concentration of mercury in parts per billion (ppb) 1. O85.3 2. O48.6 3. O79.5 4. O5.03 5. O34.6

What volume of 0.717 M HCI is required to titrate 11.9 ml of 0.151 M KOH? O a. 2.91 mL O b. 1.89 mL O C. 4.31 mL O d. 2.51 mL O e. 3.48 mL

A 1.2525 g sample of canned tuna was analyzed by the Kjeldahl method: 30.25 mL of 0.1200 N HCl was required to titrate the liberated ammonia. Calculate the % N in the sample. a. 3.25 % b. 5.32 % c. 4.06 % d. 7.46 %

0.178 L of aqueous HCl solution of unknown concentration was titrated with 0.825 M KOH (aq). 68.4 mL of the base was used to reach the endpoint of the titration. What is the concentration (M) of the acid? OA. 3.2 M O B. 0.453 M O. 0.215 M OD. 2.1 M O E. 0.317 M

Silver chloride has Ksp = 1.8 × 10−10. What is its molar solubility in water?   a. 9.5 × 10−6 M   b. 1.3 × 10−5 M   c. 9.0 × 10−11 M   d. 6.7 × 10−6 M   e. 3.6 × 10−10 M

what’s the answer for this

5. When an acid reacts with an active metal, a. the hydronium ion concentration increases. b. the metal forms anions. c. hydrogen gas is produced. d. carbon dioxide gas is produced

36. Titrating a 10.00 mL aliquot of 0.150 M NaOH with 0.120 M HCl will require a. 8.00 mL b. 0.18 mL c. 18.00 mL d. 12.50 mL

A 500 mL sample of waste water contains 15.72 µg of mercury, Hg. If the density of the sample is 1.073 g/mL. Calculate the concentration of mercury in parts per billion (ppb) 1. O 29.3 2. O48.6 3. O79.5 4. O5.03 5. O31.4

The solubility product, Ksp, for BaSO4 is 1.1 × 10–10. What is the solubility of BaSO4 in water, in moles per litre? Select one: a. 5.5 × 10–11 mol L–1 b. 1.0 × 10–5 mol L–1 c. 2.1 × 10–5 mol L–1 d. 1.1 × 10–10 mol L–1

A 1.00 liter solution contains 0.33 moles nitrous acid and 0.25 moles potassium nitrite . If 0.13 moles of hydrobromic acid are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of hydrobromic acid.) JA. The number of moles of HNO2 will remain the same. B. The number of moles of NO2 will decrease. |C. The equilibrium concentration of H30* will decrease. D. The pH will increase. E. The ratio of [HNO2] / [NO2] will remain the same.

A 60mL HCl solution is titrated with 25mL of a 0.60M KOH solution. What is the concentration of the HCl solution? a. 0.25 mol/L b. 1.56 mol/L c. 0.65 mol/L d. 2.5 mol/L

A 1 liter solution contains 0.514 M hydrocyanic acid and 0.386 M potassium cyanide. What will the addition of 0.193 moles of hydrobromic acid do? (Assume that the volume does not change upon the addition of hydrobromic acid.) *More than one answer is accepted. A. Raise the pH slightly B. Lower the pH slightly C. Raise the pH by several units D. Lower the pH by several units E. Not change the pH F. Exceed the buffer capacity

ENB Assume the densities of all solutions are 1.0 g/ml and their specific heat capacities 4.184 J/g. Experime The enthalpy change of neutralization Part I 3 NH4OH(aq) + HCl(aq)- NH4CI(aq) + H2O(E) 2.1 Equation of reaction: 2.0 M HCI 2.0 M NH.OH Volume Number of moles 0.05 25 ml 25 ml 0.05 Temperature 15 °C 15 °C eaction Initial Temperature,T Final Temperature, T Change in temperature, AT 15 °C 16.5 °C 1.5 °C Calculation of q- in J (q- = - qsa) 2.2 What is the enthalpy change (AH) in kJ.mol, when 1 mol of acid is 2.3 neutralized?

Can you help me filling all the  table with this data please I really appreciate it! Titration of Acetic Acid and Vinegar - Topic

The solubility constants, Ksp of selected fluorides are given below. Which of these compounds will be the most solubile in water? Barium fluoride 1.0 x 106. Calcium fluoride 5.3 x 109. Magnesium fluoride 3.7 x 109. Lead (II) fluoride 3.6 x 108. Select one: O a. Barium fluoride O b. Calcium fluoride O c. Magnesium fluoride O d. Lead (II) fluoride O e. The choices have equal solubilities in water.

UmL 36. For the reaction between 200.0 mL of 0.100 M silver nitrate and 95.00 mL of 0.100 M sodium chloride, the concentration of the silver ions in solution after the reaction is complete is: a. 0.00 M. All of the silver ions are used to make the precipitate. b. 0.100 M. The silver ions do not participate in the chemical reaction and are considered spectator ions. c. greater than 0.100 M. For every 1.0 mol of silver nitrate there are 2.0 mol of silver ions in the solution. d. less than 0.100 M. Even though silver ions do not react, they are diluted when mixed with the sodium chloride solution. e. less than 0.100 M. Some, but not all, of the silver ions are used to make the precipitate.

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A 500 mL sample of waste water contains 42.65 ug of mercury, Hg. If the density of the sample is 1.073 g/mL. Calculate the concentration of mercury in parts per billion (ppb) 1. 0853 2. 048.6 3. 079 5 4. O5.03 5. 034.6 Previous Next cs hp 近

5. Titrate 35.00 mL of 0.156 M KHP solution requires 25.75 mL of an unknown NaOH solution to reach the equivalence point. What’s the molarity of this unknown NaOH solution?   Group of answer choices A. 2.01 B, 0.235 C. 1.203 D, 0.212

The H+ Molarity of a 0.0150 M HNO3(aq) is estimated to be Note that HNO3 is a strong acid. A. 0.010 OB. 0.0150 O C. 1.0 OD. 1.5

1. Zia titrates 20.00 mL of an HCl(aq) solution that has an unknown concentration with 0.1240 M NaOH(aq). The equivalence point is reached after adding 25.46 mL of NaOH(aq).   a. Write out the complete balanced equation for the reaction that occurs in this titration.   b. How many moles of NaOH were added to the HCl solution?   c. How many moles of HCl were in the original 20.00 mL solution?   d. What was the concentration of HCl in the original 20.0 mL solution?

1. A series of BOD tests was run at three different dilutions. The results are shown on the table. What are the individual BOD’s? Bottle D Initial DO, mg/L Final DO, mg/L BOD, mg/L 1 100 10.0 2.5   2 200 10.0 6.0   3 400 10.0 7.5

2 20 E Solid silver fluoride is slowly added to 150 mL of a potassium chromate solution until the concentration of silver ion is 0.0538 M. The maximum amount of chromate remaining in solution is C Submit Answer $ 4 R FI F V Retry Entire Group 8 more group attempts remaining % Use the References to access important values if needed for this question. 5 T Cengage Learning | Cengage Technical Support G ^ 6 B MacBook Pro Y H & N 20 7 U N ▶II * 00 8 J I M ( 9 K O V. ) O < L ✔ M. P A Previous Email Instructor + Next Save and Exit 21 ?

While making a stock solution of NaSCN using 0.8 g of NaSCN in a 10 mL volumetric flask. 750 microliters of this solution were added to a 3500-microliter cuvette. What is the initial concentration of NaSCN in the cuvette? A. 0.21 M B. 13.18 M C. 2.82 M A. 1.07 M

Find the Final volume of buret (mL) and the Concentration of NaOH (M )

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