spaggy Posted March 12, 2020 Posted March 12, 2020 according to the balanced equation what is the answer to the problem 2HCl + Ca(OH)2 --> CaCl2 + 2H2O How many mL of 4.7 M HCl are required to neutralize (react completely) with a 868.7 mL of 4.69 M Ca(OH)2? i need some help please explain your work
swansont Posted March 12, 2020 Posted March 12, 2020 This looks like homework, so first, you explain what you've tried and why you're stuck
studiot Posted March 12, 2020 Posted March 12, 2020 You are confused ? Well so am I. Calcium hydroxide is barely soluble with a solubility product of 5.5 x 10-6 So I make its solubility as 0.0112M at room temperature. Did you copy the molarities down correctly?
Curious layman Posted March 12, 2020 Posted March 12, 2020 On 3/12/2020 at 8:49 PM, studiot said: You are confused ? Well so am I. Calcium hydroxide is barely soluble with a solubility product of 5.5 x 10-6 So I make its solubility as 0.0112M at room temperature. Did you copy the molarities down correctly? Expand Could it be a trick question?
BabcockHall Posted March 14, 2020 Posted March 14, 2020 The calcium hydroxide should come into solution as one adds more HCl. I doubt that it is a trick question.
studiot Posted March 14, 2020 Posted March 14, 2020 On 3/14/2020 at 5:18 PM, BabcockHall said: The calcium hydroxide should come into solution as one adds more HCl. I doubt that it is a trick question. Expand But where would you get a 4.69M solution of calcium hydroxide?
BabcockHall Posted March 14, 2020 Posted March 14, 2020 (edited) It would not be a true solution; it would be heterogeneous. It could be that the problem is imperfect, as opposed to being a trick question. As someone who has written my fair share of homework problems, I can say that it easy to overlook difficulties like this. Nevertheless, the amount of HCl needed to neutralize it is still something that could be calculated. Edited March 14, 2020 by BabcockHall
studiot Posted March 14, 2020 Posted March 14, 2020 On 3/14/2020 at 5:34 PM, BabcockHall said: It would not be a true solution; it would be heterogeneous. It could be that the problem is imperfect, as opposed to being a trick question. As someone who has written my fair share of homework problems, I can say that it easy to overlook difficulties like this. Nevertheless, the amount of HCl needed to neutralize it is still something that could be calculated. Expand There would be a 0.01M solution, with a quickly settling sludge in the bottom of the container. 'Imperfect' is a polite way of describing such a problem.
John Cuthber Posted March 15, 2020 Posted March 15, 2020 Did anybody specify that the solvent is water? I must admit, I can't easily think of anything in which you could prepare a 4.69M solution of Ca(OH)2
studiot Posted March 15, 2020 Posted March 15, 2020 On 3/15/2020 at 10:27 AM, John Cuthber said: Did anybody specify that the solvent is water? I must admit, I can't easily think of anything in which you could prepare a 4.69M solution of Ca(OH)2 Expand Wouldn't a different solvent also have to dissolve HCl ?
John Cuthber Posted March 15, 2020 Posted March 15, 2020 On 3/15/2020 at 11:06 AM, studiot said: Wouldn't a different solvent also have to dissolve HCl ? Expand There would be nothing to stop you using water as the solvent for the acid and a different solvent for the base- as long as the solvents mix (and no awkward side reactions happen). Maybe glycerin or glycol would dissolve enough calcium hydroxide; they are certainly better solvents than water is.
studiot Posted March 15, 2020 Posted March 15, 2020 (edited) On 3/15/2020 at 4:29 PM, John Cuthber said: There would be nothing to stop you using water as the solvent for the acid and a different solvent for the base- as long as the solvents mix (and no awkward side reactions happen). Expand That's true enough. Quote https://pubchem.ncbi.nlm.nih.gov/compound/Calcium-hydroxide#section=Solubility 0.2 % at 32° F (NIOSH, 2016) National Institute of Occupational Safety and Health. NIOSH Pocket Guide to Chemical Hazards (full website version). https://www.cdc.gov/niosh/npg (accessed August 2016). Slightly soluble in water. Insoluble in ethanol. Soluble in glycerol In water, 1730 mg/L at 20 °C PMID:2205893 Shiu WY et al; Rev Environ Contam Toxicol 116: 15-187 (1990) In water, 0.160 g/100 g water at 20 °C Haynes, W.M. (ed.). CRC Handbook of Chemistry and Physics. 94th Edition. CRC Press LLC, Boca Raton: FL 2013-2014, p. 4-55 Very slightly soluble in boiling water. Insoluble in alcohol. O'Neil, M.J. (ed.). The Merck Index - An Encyclopedia of Chemicals, Drugs, and Biologicals. Cambridge, UK: Royal Society of Chemistry, 2013., p. 292 Soluble in acid Haynes, W.M. (ed.). CRC Handbook of Chemistry and Physics. 94th Edition. CRC Press LLC, Boca Raton: FL 2013-2014, p. 4-55 Soluble in glycerol, sugar or ammonium chloride solution; soluble in acids with evolution of much heat O'Neil, M.J. (ed.). The Merck Index - An Encyclopedia of Chemicals, Drugs, and Biologicals. Cambridge, UK: Royal Society of Chemistry, 2013., p. 292 Solubility in water: none (32°F): 0.2% Expand Edited March 15, 2020 by studiot
BabcockHall Posted March 16, 2020 Posted March 16, 2020 HCl is soluble in many solvents. I used to buy a solution of at least 1 M in dioxane IIRC.
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