Wite Moteular Equation, Total ionia og uationand nat ionic egunation f he followin leactions. Reading Na co solution with HCl solution headting KCL saluition with Na co,2olutic > heading Na so, solution with BaCla sdution
Q: A solution of phthalic acid was titrated to a pH of 4.63. a. What are the 2 main species present in…
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A: Molarity (M) is the amount of a substance which is present in a certain volume of solution. The…
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Q: sample Own oncentration, with phenolphthalein as an indicator. t was titrated to the end point with…
A: Molarity is the number of moles of solute present per litre of solution.
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A: Given, Ksp = 2 x 10-47 . Volume of Solution = 100 mL 1 L = 1000 mL
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A: We know that, pH + pOH=14 If pH is less than 7 then solution is acidic.
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A: The explanation is given below-
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Q: what Volume in milliiters 12.0M HCl 8olution is nzeded do prepase 250.0 me goluti on at O.50OM? of a…
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A: Given:-Volume of H2SO4=10.0cm3=10.0×10-3L as 1cm3=10-3LMolarity of H2SO4=0.100MVolume of NaOH=25.0…
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Q: Which of the following is true regarding acids and bases? a. All Bronsted-Lowry bases are…
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Q: Question attached
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Q: A 15.00mL sample of ammonium hydroxide (0.980g/mL) is titrated with 31.25mL of 0.500M HCl. Find the…
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Q: The molar solubility of calcium phosphate in a 0.196 M ammonium phosphate solution is M. Submit…
A: Formula of calcium phosphate is Ca3(PO4)2 Formula of ammonium phosphate is (NH4)3PO4
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A: In pure water AgI have greatest solubility.
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Q: solution only represent the end po of titration. * O True O False
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- A public water supply was found to contain 0.8 partper billion (ppb) by mass of chloroform, .(a) How many molecules would be present in a350 mL glass of this water? (b) If the in part (a)could be isolated, would this quantity be detectable onan ordinary analytical balance that measures masswith a precision of g?An aqueous solution of acetic acid with a richness of 80% by passage (ρ = 1.07 kg/dm3) is available.a) What is the molarity and molality of this solution?b) What is the percentage of acid in this solution? c) What volume of said solution should we use to prepare 1 liter of 2.14M solution?Stock phosphoric acid solution is 85% H3PO4 and has a specific gravity of 1.70 . Hence, the molarity of H3PO4 solution that is prepared by diluting 15.0 mL aliquot of H3PO4 stock solution to 135 mL H2O is?
- The freezing point of a 0.100 M acetic acid (CH3COOH) solution is determined to be-0.1878 C. Estimate the percent dissociation of acetic acid in this solution. Is it a strong orweak electrolyte? Note that acetic acid produces acetate (CH3COO-) and hydrogen (H+) ionswhen it is dissolved in water.Prepare 0.1 M solutions of NaOH and 0.1 M ethyl acetate using high-purity distilled water. So, weight desired amount of NaOH and ethyl acetate and dissolved in dH2O to prepare stock solution in equal molarity. Mw (NaOH) = 40.0 g/mol , Mw (EtOAc)= 88.1 g/mol, Density(EtOAc): 0.898 g/cm325 mL of a bleach (NaOCl) sample is diluted to 500 mL. An excessive amount of KI is added to the 20 mL solution taken from here and the I2 released is titrated with 35.5 mL of 0.0409 M NaS2O3. Accordingly, calculate the weight percent by volume of NaOCl in the sample. (MaNaOC:74,4 g/mol)
- To what final volume should you dilute 50.0 mL of a5.00 M KI solution so that 25.0 mL of the diluted solutioncontains 3.25 g of KI?The Henry’s law constant for CO2 in water at 25 °C is3.1x 10-2 M atm-1. (a) What is the solubility of CO2 inwater at this temperature if the solution is in contact withair at normal atmospheric pressure? (b) Assume that all ofthis CO2 is in the form of H2CO3 produced by the reactionbetween CO2 and H2O:CO2(aq) + H2O(l)------>H2CO3(aq)What is the pH of this solution?How many grams of GaAs04 are required to prepare 2800 mL. of dissolution 0.035 N. ?
- How many milligrams of solid MgCl2 (Formula Weight: 95.211 g/mole) are required toprepare 250mL of a 150mM solution?How many moles of solute particles are present in 1.64 mL of 0.458 M K2SO4? (the answer is 2.25E-3 but i would appreciate some insight on what steps to take!)It is sometimes asserted that carbonates are soluble instrong acids because a gas is formed that escapes (CO2).Suppose that CO2 were extremely soluble in water (as, forexample, ammonia is) and therefore it did not leave thesite of the reaction, but that otherwise, its chemistry wasunchanged. Would calcium carbonate be soluble in strongacids? Explain.