Q: Calculate the pH of a solution containing 0.75 M lactic acid (ka = 1.4 x 10-4) and 0.25 M sodium…
A: pKa = -log Ka pKa = - log (1.4 x 10-4 ) = 3.85 pH of an acidic buffer solution: pH = pKa + log…
Q: A unsaturated aqueous so
A: Needed formulas are 1. Ca(OH)2 --> Ca+2 + 2 OH- Ksp =…
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A: Answer. A solution containing highest amount of solute is called a saturated solution. A saturated…
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A: Solubility product values - SrF2 =4.33×10-9SrCO3=5.60×10-10SrSO4 =3.44 ×10-7
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Q: Calculate AG for the dilution of aqueous HCl from 2.17 M to 0.276 M at 25°C.
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Q: Calculate the volume (mL) of 0.100 M H3PO4 required to neutralize 25.0 mL of 0.010 M Ca(OH)2.
A: Given:Molarity of H3PO4 is 0.100 M.Volume of Ca(OH)2 is 25.0 mL.Molarity of Ca(OH)2 is 0.010 M.
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Q: A solution containing 2.00 mol Ca(OH)2 is titration with HCl. How many miles of HCl are required to…
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Q: What volume of 0.0105 M HBr solution is required to titrate 125.0
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Q: True or False. Write TRUE if the statement is correct and FALSE if it is incorrect.…
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Q: How many liters of pure water will be requried to disslove 0.885 grams of solid Lead iodate,…
A: The solubility reaction of solid Lead iodate can be written as
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A: Using Henderson hasselbalch equation:-
Q: An aqueous solution is 0.0155 M in iron (II) ammonium sulfate. Fe(NH4)2(SO4)2. Calculate the net…
A: When a strong electrolyte is added to the solution, it undergoes complete dissociation. So the total…
Q: A 45.0 ml sample of 0.250 M CH3CH2NH2 was mixed with 32.0 mL of 0.225 M HNO3. Kp = 5.6 x 104 %3D а.…
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Q: A 45.0 mL sample of 0.250 M CH3CH2NH2 was mixed with 32.0 mL of 0.225 M HNO3. Kb = 5.6 x 104 %3D a.…
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Q: Calculate the percent ionization of 0.0080 MM butanoic acid (Ka=1.5×10^−5).
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A: Molarity of NaOH = 0.100 M Volume of NaOH = 32.50 mL Molar mass of Acid = 180.16 g/mol
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Q: An instrument used to measure the acidity or alkalinity of a solution.
A: As per bartleby guidelines I answered only first question so please don't mind.Thanks in advance.
Q: For the titration of 50.00 mL of 0.106 M NH3 with 0.225 M HCl, calculate the pH when neutralization…
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Q: An unknown hydroxide of the formula X(OH)2 is only slightly soluble in water. She takes 25.00 mL…
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Q: Titration of a 86.00mL KOH solution required 398.00 ml of 0.0240 M acetic acid. What is the molarity…
A: )
Q: Calculate the [Y"] in a saturated solution of YF3 in 0.003150 M NaF(). (Kap for YF3 = 8.6 x 10") %3!
A: Solubility product (Ksp) is defined as the products of ions present in a solution of a salt.
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Q: Calculate the ionic strength of a solution of 0.10 M KCl.
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Q: How many MILLILITERS of lactic acid and GRAMS of sodium lactate must be added to 1L of water to…
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Q: What is the pH value of saturated lime (Ca(OH)2) solution? (Ksp =Kb=8x10 -10)
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Q: 2. The reaction utilized in Part I of the experiment is: НС-Н,О2(ад) + NaOH (aq) — Н,0 () + C-H;О2…
A: The reaction taking place in the experiment is, HC2H3O2 (aq) + NaOH (aq)→H2O (l) + C2H3O2-(aq)
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Q: Consider the titration of 300.0 mL of 0.500 M NH3 (Kh = 1.8 x 105) with 0.500 M HNO3. What is the pH…
A: Mnmn
Q: Calculate the molar ionic strength of a 0.5800 M copper (III) sulfide solution.
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Calculate hardness of water if water sample contains Ca(HCO3)2=40ppm
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- How many liters of pure water will be requried to disslove 0.885 grams of solid Lead iodate, Pb(IO3)2? Ksp=2.5x10^-13What is the pH of the solution after mixing 0.171 g of Mg(OH)2 (MW=58.321 g/mol) with 68.9 mL of 0.0569 M HCl? The resulting solution was diluted to 100 mL. Round your calculated value for pH to two figures to the right of the decimal point.A tablet contains 0.5 g of magnesium hydroxide as the only basic ingredient . The tablet is analysed by dissolving it and titrating with a standard hydrochloric acid solution .The hydrochloric acid solution used in this titration is made by diluting 200 ml of 2M standardised solution to 500 ml 1.Calculate the volume of the HCl solution required to neutralize two of these indigestion tablets dissolved in water to make 35ml solution and calculate the concentration of Cl- in the final solution in mol.dm-3
- Calculate the mass (in g) of solid sodium hydroxide (molar mass = 39.997 g/mol) required to prepare: 5 litres of a solution with pH 12.4. 85 mL of a 2.60 M solution. 250 mL of 50 % (w/w) solution. The density of 50 % (w/w) NaOH is 1.515 g/mL.calculate the equivalence point volume in the containter of 2.00 g Ba(OH)2 with 0.100 M HCl. molar mass of Ba(OH)2 = 171.3 g/molExplain why the conductivity of mixture A is higher than that of mixure B, , yet the pH of A is lower than the pH of B. Include relevant equations in your answer B 0.1 mol L–1 CH3COOH Conductivity (mA) 5 PH 3 A 0.1 mol L–1 HCl 260 1
- H2. Titrations are performed by a scientist in the laboratory as follows: a solution of deuterated hydrochloric acid contains 1.08 g DCl in 750 ml of deionised, distilled water. An average amount of 14.95 ml of the DCl(aq) solution is titrated with 25.0 ml of Ca(OH)2 to produce an endpoint (as determined by an appropriate indicator). What is the molarity of the Ca(OH)2 solution? You must include all of your calculations Please give typed answerCaculate the pH of a solution prepared by mixing 84.7 mL of a 0.25 M aqueous aniline solution (C6H5NH2, Kb = 4.3 x 10-10) with 100. mL of a 0.11 M aqueous nitric acid solution. Your pH should be reported to two places past the decimal point.Answer the following questions about calcium hydroxide, Ca(OH)2(s). A student makes a saturated solution of calcium hydroxide, as shown below, using DI water at a temperature greater than 25 °C.Ca(OH)2(s)⇌ Ca2+(aq) + 2 OH –(aq) a.The pH of the saturated solution is 11.611. Determine the [OH−]. b.Determine the Ksp of Ca(OH)2(s) for this solution. c.The Ksp of Ca(OH)2(s) at 25 °C is 6.5 x 10−6. Does the solubility of Ca(OH)2(s) increase, decrease, or remain the same at solvent temperatures greater than 25 °C? Justify your answer.
- An aqueous solution is 0.0155 M in iron (II) ammonium sulfate. Fe(NH4)2(SO4)2. Calculate the net ionic strength,u, of the solution.1. An acid solution is prepared by dissolving 19.264 grams of pure KHC2O4.H2C2O4.2H2O in water and diluting to exactly 900 ml. Fifty milliliters (50.00 mL) of this solution are neutralized by 35.00 ml. of KOH solution. What is the normality of each solution? 2. What mass of Ca(OH)2 is present in a sample if it is titrated to its equivalence point with 44.02 mL of 0.0885 M HNO3? The balanced chemical equation is as follows: 2HNO3 + Ca(OH)2 → Ca(NO3)2 + 2H2O ; Balanced.How many MILLILITERS of lactic acid and GRAMS of sodium lactate must be added to 1L of water to produce a solution with pH 3.9 and a total solute concentration of 1 mM? (MW Salt = 112.06; MW Acid = 90.08)