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![Thus. 1 - 0.0010 [Ca 2+ ] [sou akso 0.0010 [sour] > 6.18105 [sou ] } 6.18155 [Son] 20.061 m. 20.061 mol since volume is not c](http://img.homeworklib.com/questions/9fd439b0-78e0-11ea-86a6-d5886d1099ae.png?x-oss-process=image/resize,w_560)
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The Ksp of CaSO4 is 6.1x10-9. For 1.0 L of a 0.0010 M Ca(NO3), solution, how...
Question 30 (2.5 points) How many moles of Ca(NO3)2 must be added to 1.0 L of...
Question 30 (2.5 points) How many moles of Ca(NO3)2 must be added to 1.0 L of a 0.203 MKF solution to begin precipitation of CaF2? For CaF2, Ksp = 4,0 10-11 4.9 x 10-16 02x10-10 O 16 x 10-12 09.7x10-46 3.1 10-6
How many moles of nitrate ion are in 1.0 L of a 8.8 M Mg(NO3)2 solution?
How many moles of nitrate ion are in 1.0 L of a 8.8 M Mg(NO3)2 solution?
3 pts Question 34 As a mixed 1.0-L solution that is 0.10 M in each of...
3 pts Question 34 As a mixed 1.0-L solution that is 0.10 M in each of Ba(NO3)2 Ca(NO3)2 and Pb(NO3)2 has 0.0050 M Na Cro4 added dropwise to it, which would precipitate first? OCacro OPbCros BaCro O none of these would precipitate, they are soluble salts
Consider 1.0 L of a solution which is 0.80 M HF and 0.55 M NaF (K...
Consider 1.0 L of a solution which is 0.80 M HF and 0.55 M NaF (K for HF - 7.2x104). Part 1 Calculate the pH of this solution. pH- Part 2 Calculate the pH after 0.10 mol of HCl has been added to the original buffer solution. Assume no volume change on addition of HCI. pH- Part 3 Calculate the pH after 0.20 mol of NaOH has been added to the original buffer solution. Assume no volume change on addition...
A)A volume of 46.2 mL of a 0.568 M Ca(NO3)2 solution is mixed with 75.5 mL...
A)A volume of 46.2 mL of a 0.568 M Ca(NO3)2 solution is mixed with 75.5 mL of a 1.496 M Ca(NO3)2 solution. Calculate the concentration of the final solution. Calculate the molarity of each of the following solutions. (b) 7.25 g of methanol (CH3OH) in × 102 mL of solution: mol/L (c) 9.68 g of calcium chloride (CaCl2) in 2.20 × 102 mL of solution: mol/L (d) 8.57 g of naphthalene (C10H8) in 85.2 mL of benzene solution: mol/L
Isnt the molar solubility of Ca(OH)2 with added CaCl2 supposed to be less than the molar solubili...
isnt the molar solubility of Ca(OH)2 with added CaCl2 supposed
to be less than the molar solubility of Ca(OH)2 by itself? where
did I mess up?
A. Molar Solubility and Solubility Product of Calcium Hydroxide メーーー Desk No. Trial 1 Trial 2 Trial 3 1. Volume of saturated CalOHD, solution (ml) 2. Concentration of standardized HCI solution (mol/L) 3. Buret reading, initial (mL) . 4. Buret reading,final(mL) 5. Volume of HCI added (mL) 6. Moles of HCl added (mol) 7....
A student adds 0.0035 mol of NaF to 1.00 L of 0.02 M barium nitrate, Ba(NO3)2....
A student adds 0.0035 mol of NaF to 1.00 L of 0.02 M barium nitrate, Ba(NO3)2. Which of the following statements is correct? Ksp = 1.5 × 10–6 for BaF2. Assume there is no volume change upon addition of NaF. One must know Ksp for barium nitrate to make a determination Barium fluoride precipitates until the solution is saturated. The solution is unsaturated and no precipitate forms. The solubility of barium fluoride is increased upon the addition of fluoride ions....
A solution of 0.1 L of 0.3 M Ca(NO3)2 is mixed with 0.2 L of0.06...
A solution of 0.1 L of 0.3 M Ca(NO3)2 is mixed with 0.2 L of 0.06 M NaF. Calculate the reaction quotient Qsp. Does calcium fluoride precipitate? (Ksp (CaF2) = 3.2×10–11). (A) Qsp = 1.6×10–4; no precipitate. (B) Qsp = 1.6×10–4; a precipitate will form. (C) Qsp = 3.2×10–11; no precipitate. (D) Qsp = 3.2×10–11; a precipitate will form. (E) Qsp = 3.2×10–7; no precipitate.
is this graph right? and how to get the ksp? Adding Ca(NO3)2 to NaOH 9. On...
is
this graph right? and how to get the ksp?
Adding Ca(NO3)2 to NaOH 9. On the report, number twelve (12) wells on the spot plate consecutively 1 - 12. In wells 2- 12, carefully count 10 drops of purified water into each well. All wells 2-12 will now contain 10 drops of water. 10. In well 1. place 10 drops of the 0.10 M NaOH solution. 11. In well 2, add 10 drops of the 0.10 M NaOH solution....
How many moles of sodium hypobromite (NaBrO) should be added to 1.00 L of 5.5×10^?2 M...
How many moles of sodium hypobromite (NaBrO) should be added to
1.00 L of 5.5×10^?2 M hypobromous acid (HBrO) to form a buffer
solution of pH= 9.17? Assume that no volume change occurs when the
NaBrO is added. I posted this question previously but it was
answered incorrectly
How many moles of sodium hypobromite (NaBrO) should be added to 1.00 L of 5.5*10-2 M hypobromous acid (HBrO) to form a buffer solution of pH=9.17? Assume that no volume change occurs...
Question 30 (2.5 points) How many moles of Ca(NO3)2 must be added to 1.0 L of a 0.203 MKF solution to begin precipitation of CaF2? For CaF2, Ksp = 4,0 10-11 4.9 x 10-16 02x10-10 O 16 x 10-12 09.7x10-46 3.1 10-6
3 pts Question 34 As a mixed 1.0-L solution that is 0.10 M in each of Ba(NO3)2 Ca(NO3)2 and Pb(NO3)2 has 0.0050 M Na Cro4 added dropwise to it, which would precipitate first? OCacro OPbCros BaCro O none of these would precipitate, they are soluble salts
Consider 1.0 L of a solution which is 0.80 M HF and 0.55 M NaF (K for HF - 7.2x104). Part 1 Calculate the pH of this solution. pH- Part 2 Calculate the pH after 0.10 mol of HCl has been added to the original buffer solution. Assume no volume change on addition of HCI. pH- Part 3 Calculate the pH after 0.20 mol of NaOH has been added to the original buffer solution. Assume no volume change on addition...
isnt the molar solubility of Ca(OH)2 with added CaCl2 supposed
to be less than the molar solubility of Ca(OH)2 by itself? where
did I mess up?
A. Molar Solubility and Solubility Product of Calcium Hydroxide メーーー Desk No. Trial 1 Trial 2 Trial 3 1. Volume of saturated CalOHD, solution (ml) 2. Concentration of standardized HCI solution (mol/L) 3. Buret reading, initial (mL) . 4. Buret reading,final(mL) 5. Volume of HCI added (mL) 6. Moles of HCl added (mol) 7....
is
this graph right? and how to get the ksp?
Adding Ca(NO3)2 to NaOH 9. On the report, number twelve (12) wells on the spot plate consecutively 1 - 12. In wells 2- 12, carefully count 10 drops of purified water into each well. All wells 2-12 will now contain 10 drops of water. 10. In well 1. place 10 drops of the 0.10 M NaOH solution. 11. In well 2, add 10 drops of the 0.10 M NaOH solution....
How many moles of sodium hypobromite (NaBrO) should be added to
1.00 L of 5.5×10^?2 M hypobromous acid (HBrO) to form a buffer
solution of pH= 9.17? Assume that no volume change occurs when the
NaBrO is added. I posted this question previously but it was
answered incorrectly
How many moles of sodium hypobromite (NaBrO) should be added to 1.00 L of 5.5*10-2 M hypobromous acid (HBrO) to form a buffer solution of pH=9.17? Assume that no volume change occurs...
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