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 20.0 mL sample of an HCl solution is titrated with 27.4 mL of a standard solution of Ba(OH)2. The concentration of the standard is 0.0154 M. What is the molarity of the HCl?    a. 4.22 M b. 42.02 M c. 0.0422 M d. 0.422 M

Solubility of PbCl2 in water is 0.0150 g/L at 25 oC.  What is the molar concentration of             Cl- ion in the solution at the same temperature?     A. 3.30 x 10-3 M   B. 5.40 x 10-5 M   C. 1.08 x 10-4 M   D. 3.10 x 10-4 M   E. 1.10 x 10-2

At a certain temperature, the solubility of Pbl, in water is 1.5 x 10-3 mol /liter. Based on that, the Ksp Pbl2 is Oa. 6.75 x 10-8 b. 4.50 x 10-8 c. 4.50 x 10-9 O d. 3.37 x 10-9 e. 1.35 x 10-8 e Next page

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 %

A 1.00 liter solution contains 0.52 moles hypochlorous acid and 0.40 moles potassium hypochlorite. If 0.20 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.) A. The number of moles of HC1O will decrease. ⒸB. The number of moles of C10¯ will remain the same. C. The equilibrium concentration of H3O+ will decrease. ⒸD. The pH will remain the same. [HCIO] [C10¯] ⒸE. The ratio of will increase.

what’s the answer for this

A 1.047 g sample of canned tuna was analyzed by the Kjeldahl method; 24.61 mL of 0.1130 M HCI were required to titrate the liberated ammonia. Calculate the percentage of nitrogen in the sample. 1. 03.89% 2. 0299% 3. 039 9% 4. 09.38% 5. 02.10% Previous Next CS hp

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 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?

Consider the reaction NH3(aq) + H₂O(2) NH4+ (aq) + OH(aq). Kb for NH3 is 1.8 x 10-5 at 25°C. What is Ka for the NH4* ion at 25°C? O a. 9.2 x 10-8 O b. 1.8 x 10-5 O c.7.2 x 10-12 O d. 5.6 x 10-10 5.6 × 104 O e.

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

In an experiment, a 500.0 mL solution of approximately 0.250 M KOH (56.106 g/mol) solution was prepared. The actual concentration was then determined by standardizing against 1.0050 g of KHP(204.22 g/mol), which required 19.45 mL of the KOH solution. One mole of KOH reacts with one-mole ofKHP.a.How would you prepare the KOH solution?b.After standardization, what will be the exact molarity of the KOH solution?c.The KOH solution was then used to analyze a sample containing oxalic acid, H2C2O4 (90.03g/mol). If the titration required 11.33 mL KOH, how many grams of oxalic acid is in the sample? Oxalic acid releases two protons during the reaction.

5. If magnesium hydroxide were used instead of NaOH, how many moles would it take to combine with three moles of KHP? Explain.

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

A 25.0mL acetic acid sample was titrated using exactly 69.72 mL of a 0.30M sodium hydroxide solution until the endpoint was achieved. What is the molar concentration of the acid sample? A. 0.02 M B. 0.98 M C. 1.95 M D. 3.90 M E. 9.76 M

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?

If there are 2.0 mg of Pb+2 ions in 1.0 L of water, what is the concentration of lead in ppm? a. 200 ppm b. 20. ppm c. 0.0020 ppm d. 2.0 ppm e. 0.20 ppm