Ch 10.2 practice worksheet

Help with the following question. Ksp for Co(OH)2 is 5.02 x 10^-6

How does the heat or enthalpy of the reaction (ΔHrxn) change when the concentration of a Strong acid (HCl) is increasing and the concentration of strong base (NaOH) is kept constant in a solution mixture? plz answer showing the steps to solve quantatiavely using hess's law. ive also attached images of my lab data for reference

aosdnag given required solution type only

Part E Write balanced complete ionic equation for NaOH(aq)+ HC,H,O2 (aq)→H,O(1) + NaC, H,O2 (aq). Express your answer as a chemical equation. Identify all of the phases in your answer. ΑΣΦ x" O That's not quite right. Please check your formatting and try again No credit lost. Try again. Submit Previous Answers Request Answer Part F Write balanced net ionic equation for NAOH(aq) | HC,H,O, (aq) H,O(1) i NaC, H,O, (aq). Express your answer as a chemical equation. Identify all of the phases in your answer.

I need help with the calculations to fill in the data table

What is the Mass of solvent in grams? Add together the masses of the liquid water and ice added to the calorimeter. Convert the volume of liquid water to mass using 1.000 g/mL as the density of water (see procedure for volume used). Side note:Molarity of the solution is  0.76612903225806

1) Listen -5 The Ksp value for calcium sulfate [CaSO4] is 2.40 X 10 and a professor made 1825 mL of a CaSO4(ag) solution but then one of his graduate student accidentally poured in a 0.125 M solution of calcium phosphate [Cag(PO4)2] solution. You may ignore the additional volume coming from the Ca3(PO4)2 solution to make the calculation simpler. Calculate the new sulfate (SO42) ion concentration at equilibrium with this common ion effect. 6.40 x 10-5 5.25 x 10-5 6.21 x 10-5 5.44 x 10-5 201591..docx LAB EXP. #3 -..docx Show All

A 95.0 wt% solution of ethanol (CH3CH2OH, FM 46.07) in water has a density of 0.804 g/mL. (a) Find the mass of 1.00 L of this solution and the grams ofethanol per liter. (b) What is the molar concentration of ethanol in this solution?

Iron(III) hydroxide (MM = 106.87 g/mol) has a Ksp of 6.3 x10-38.  If 35.9 g Fe(OH)3 is stirred into 6,034.63 L H2O, how many micrograms of iron(III) hydroxide will dissolve?Report your answer to the nearest whole number.

Part 2 Data Mass of Urea (g): Buret Initial Volume (mL): water Part 2 Calculation: 4.05819 24.90 A. Find the Keq for dissolving urea (saturated solution) Mass of urea used 4.05819 Moles urea = Final Temperature of saturated solution ("C): Buret Final Volume (ml): fikcal - In 1.Write the chemical equation for urea dissolving: CityN₂0 (s) + H₂0 (1) → (H₂N₂O) (aq) Volume in Liters = 2.Calculate the molarity of the urea, [Urea]eam for the saturated solution of urea in water. You must first find the moles of urea (molar mass 60.05 g/mol). Then you must use the volume given in the data (above) to find the molarity of the urea in the saturated solution. Show calculations here. 3. Calculate AG soln Volume of water used: 3.88 ML Molarity of saturated solution (NOTE: this molarity = Keq ) = To do this, use: AG soln = - RT In Keq AH-TAS soln 4. Calculate AS soln Use: AG First, re-arrange the equation given above to solve for AS soln 6 27.0 W AS soln AGOsoln Then plug in the values you got for AG°…

You are taking a road trip in a car without A/C. The temperture in the car is 85 degrees F. You buy a cold pop at a gas station. Its initial temperature is 45 degrees F. The pop's temperature reaches 60 degrees F after 47 minutes. Given that T-A -kt = e To- A where T the temperature of the pop at time t. To the initial temperature of the pop. %3D the temperature in the car. k a constant that corresponds to the warming rate. and t= %3D the length of time that the pop has been warming up. How long will it take the pop to reach a temperature of 79.75 degrees F? minutes. It will take

A solution of potassium hydroxide KOH was prepared by dissolving 1g of it in 100ml of distilled water. If you know that the water density is 1g / ml, calculate: 1. The molar focus 2. Molar concentration

Complete the following table by calculating values for the two serial dilutions

I need help with questions 1-4? Also if I'm wrong on question 1 can you do it again? If not you can continue with questions 2-4?

Ethanol has a density of 0.79g/ml. Will the 80%w/v of ethanol in water contain a higher amount of ethanol than 79%v/v? Please show solvings and explanation

What is the boiling point of a solution prepared by dissolving 251 g of octasulfur (Sg, Molar mass = 256.5 g/mol) in 2,383 g of CCI4? Kb 5.05°C/m, boiling point of pure CCI4 = 76.7°C)? Your Answer: Answer units

In the below problem I converted 50g of HCl to 1.37mol. But I'm not sure what do with that bumber and the q_system value of 670 that I got.

I need help on questions 1-2? If you can't help me on question 2, then you can help me on question 1.

The Ksp value for calcium sulfate [CaSO4] is 2.40 X 10-5 so if a professor made 1825 mL of a CaSO4lag) solution then how many grams of sulfate (SO42) ion would be present in this solution. 0.8345 gram SO42- ion 0.8588 gram SO42- ion 0.9331 gram SO42- ion 1.0036 gram SO42- ion 0.8921 gram SO42- ion 2.. 591..docx W- LAB EXP. #3 -.docx Show All

José performs an experiment to determine how much sugar can be dissolved in 250 milliliters (mL) of water at 25°C. He adds 50 grams (g) of sugar at a time to the water while stirring and observes the solution After adding sugar the eleventh tene (550 g), he notes that undissolved sugar has settled to the bottom of the container. He stops adding sugar and ends his experiment. In his lab write-up he concludes that the solubility of sugar in water at 25°C is 500 g per 250 ml. is his conclusion defensible, and why or why not? O No, because he did not add sugar enough times. Yes, because when he added more than 500 g it did not all dissolve. O No, because he does not know if any of the final portion of sugar dissolved. O Yes, because when he added the tenth portion (500 g) all of it dissolved.

Standardization of a sodium hydroxide (NaOH) solution against potassium hydrogen phthalate (KHP) yielded the following results: Mass of KHP, g Volume of NaOH, mL 0.7987 38.29 0.8365 38.96 0.8104 38.51 0.8039 38.29 MM KHP: 204.22 MM NaOH: 40.00 a. Calculate the mean molar concentration of sodium hydroxide. (First, compute the concentration of NAOH in each titration then compute for its mean/average value.) b. Calculate the standard deviation. Please provide solutions for your answers. If you have used your calculator for calculating for mean and standard deviation, you can just provide the formula with the values indicated.

A solution is prepared by dissolving 24.5 g of CaCl2 (MW = 110.98 g/mol) in 385 mL of water. The density of the resulting solution is 1.05 g/mL. The concentration of CaCl2 in this solution is molar. Answer accurate to three decimal places. Your Answer: Answer