Calculate the equilibrium concentration of Ni²* in a solution with an analytical NİY2- concentration of 0.0100 M at pH 2.0 and pH 9.0. K; of NIY2= 4.2 x 1018

Q: If you needed to perform a reaction in a controlled pH environment that was fairly basic, you might…

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Q: If a water has a carbonate alkalinity of 120.00 mg/L as the ion and a pH of 10.30, what is the…

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Q: A 0.3654 g portion of pure formic acid (CH2O2, FW=46.03 g/mol, Ka=1.77 x 10-4) is dissolved in 50.00…

A: Given that, Mass of formic acid = 0.3654 g Molecular mass of formic acid = 46.03 g/mol Volume of…

Q: 7.) The K, of an acid is determined to be 0.00589. What is the pK,.

A: PKa = -log(Ka)  This is the relation between Ka and pKa is

Q: a) Calculate the pH of a buffer hat has 0.055 M HCIO and 0.034 M Naclo. The K, for HCIO is 2.9x10*.…

A: The Henderson-Hasselbalch equation for determination of pH is,

Q: 2. Calculate the pH of water at 25°C and 75°C. The values for pKw at these temperatures are 13.99…

A: 2. Solution - According to the question - Given - 1. At 25 °C 2H₂O ⇌ H₃O⁺ + OH⁻ pH = ½pKw = ½ ×…

Q: Calculate the pH at the second stoichiometric point when 170 mL of a 0.015 M solution of amber acid…

A: Volume of NaOH required to reach the second equivalence point can be calculated as:…

Q: The normal pH of blood is 7.40 6 0.05 and is controlled in part by the H2CO3/HCO3- buffer system.(a)…

A: Given: The pH of the blood= 7.20 The Ka for the carbonic acid=4.5 * 10-7.

Q: What will be the pH of a buffer solution containing an acid with a pKa of 5.4 with an acid…

A: We have to predict the pH of buffer solution.

Q: The following observations are made about a diprotic acidH2A: (i) A 0.10 M solution of H2A has pH =…

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Q: 500ml of a 0.1M sodium phosphate buffer with pka of 7.21is diluted. Calculate the pH of of the…

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Q: alculate the pH of a solution obtained by m plumes of formic acid and sodium hy- ncentration of 0.2…

A: Ka = 2.04 ×10-4 pKa = -log(Ka)   = 3.69 At same concentration of acid and base ,it forms salt.

Q: Given a theoretical acid, HA, with a pKa of 6.52. Calculate the pH of 30.0mL of 0.400M HA, when it…

A: The total number of HA acids in the solution is determined below. nHA=MHA×VHA=0.400 mol/L×30.0…

Q: The pH of 0.65 M aqueous solution of a weak base (monoprotic) is 10.24. Determine the pKp of this…

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Q: The concentration of total phosphorous (HPO4^2- and H2PO4^-) found in a blood sample is determined…

A: Henderson - hasselbach equation enables the calculation of pH of a buffer solution made by mixing…

Q: Benzoic acid (C₂H5CO₂H), a weak acid, has a dissociation constant of K=6.3x10^-5.   1. Write the…

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Q: A buffer solution is 0.452 M in HClO and 0.357 M in KClO . If Ka for HClO is 3.5×10-8 , what is the…

A: Note : Since you have posted multiple questions, we are entitled to answer the first only. Please…

Q: calculate the pH of a solution that is 1.00 M CH3COOH (ka = 1.0 x 10^-5) and 1.00 M CH3COONa

A: Given: Concentration of weak acid CH3COOH = 1.00 M And the concentration of CH3COONa = 1.00 M

Q: Consider the reaction of 75.0 mL of 0.350 M C₅H₅N (Kb = 1.7 x 10⁻⁹) with 100.0 mL of 0.393 M HCl.…

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Q: Calculate the pH of a solution that is 0.200M in NH3 and 0.300M in NH4Cl. The dissociation constant…

A: Given: Concentration of NH3 = 0.20 M Concentration of NH4Cl = 0.30 M Kb = 1.75x10-5

Q: Sketch a plot of the fraction of species, f, vs pH for Tyr. Show your calculations for several…

A: Answer -

Q: A chemist titrates 170.0 mL of a 0.1735M pyridine (C,H,N) solution with 0.3504M HBr solution at 25…

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Q: Use the Henderson-Hasselbalch equation to calculatealculate the pH of the solution prepared by…

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Q: Calculate the pH of a 1.07 M solution of a weak acid, AH, for instance CH3COOH, and 0.62 M of a…

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Q: Ethylamine (C2H5NH2) has a Kb value of 4.5x10–4. Calculate the pH of a buffer solution that is…

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: What is the pH of a solution of 0.400 M CH3NH2 containing 0.300 M CH;NH3I? (Kb of CH3NH2 is 4.4 ×…

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Q: A student needs to prepare a buffer solution with a pH of 5.26. Assuming a pKa of 4.73, how many mL…

A: A buffer solution is the one which is formed by mixing “a weak acid with the solution of the salt of…

Q: Given that the Kf for [Ni(H2O)5(NH3)]2+ is 501 and Ka for NH4+ is 2.0 x 10-5, what is the…

A: Given data, Ka for NH4+=2.0×10-5Kf for [Ni(H2O)5(NH3)]2+=501

Q: The acid- dissociated constant at 25.0 degres celcius for hypochlorous acid (HCIO) is 3.0x10-8. At…

A: We are given that the acid-dissociation constant for hypochlorous acid is 3.0 × 10-8, and the…

Q: Weighed quantity of dry potassium bromide 1,5560 gr (M=167,000 g/mol) dissolved in water with…

A: Measuring the quantity of a solution of a known concentration of titrant that is needed to react…

Q: v. What is pH? Calculate the pH for 0.0001N NH4OH solution of 100mL volume. The pKb value for NH4OH…

A: Ammonium hydroxide is a weak base. The dissociation of the weak base is given by: NH4OH ↔ NH4+ + OH-…

Q: A diprotic indicator H2L has pK,1 of 3.5 and pK2 = 7.5. At pH = 6.0, what is the principal species…

A: The reaction would be:H2L ⇋ HL- + H+    { for  pKa2=7.5  }So,HL- is released in the solutionandH2L ⇋…

Q: Commercial phosphate buffers are sold to maintain fish tanks at a pH of 7. Use a table of acid…

A: Acid dissociation equilibrium constants for H3PO4 are :  Ka1 = 7.2 x 10-3  Ka2 = 6.8 x 10-8  Ka3 =…

Q: Why is the equilibrium between the acid NaH2PO4, and its conjugate base Na2HPO4, a suitable buffer…

A: When a solution is referred to as a weak acid or weak base, it means that the solution can undergo…

Q: Calculate the pH of a solution that is 0.279 M  acetic acid and 0.190 M  sodium acetate.The Ka of…

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Q: Kb for methylamine at 25°C is 4.4 x 10-4 what is its pH if 0.10M solution is used.

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Q: Calculate the pH of the solution made by adding 0.50 mol of HOBr and 0.30 mol of KOBr to 1.00 L of…

A: Given,  Moles of HOBr = 0.50 moles Moles of KOBr = 0.30 moles Volume of water = 1.00 L Ka for HOBr =…

Q: Given that the Kf for [Ni(H2O)5(NH3)]2+ is 501 and Ka for NH4+ is 2.0 x 10-5, what is the…

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Q: What is the mole ratio of sodium acetate to acetic acid in abuffer with a pH of 5.75?

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Q: Calculate the pH of a 0.26 M solution of a weak acid, AH, for instance CH3COOH, and 1.01 M of a…

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Q: What is the pH of a buffer solution that contains 0.245 M weak acid and 0.450 M of the conjugate…

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Q: The pH at 10, 100, and 110% titration (% of the equivalence point volume) for the titration of…

A: Solutions                           Given that the pH at 10, 100, 110% titration.

Q: The ionic compound AX3 forms a saturated aqueous solution at 25 oC when the concentration is 7.30E-4…

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Q: A 15 mL sample of water from the lemur exhibit required 3.95 mL of a sulfuric acid titrant to reacht…

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Q: To rule out metabolic acidosis in a patient's blood sample, the total carbon dioxide content should…

A: Henderson-Hasselbach equation. this equation shows the relationship between pH of a solution, the…

Q: Calculate the pK, of hypobromous acid from its K, value.

A: Since you have posted multiple questions, we are entitled to answer the first only.

Q: Calculate the pH of a solution that is 0.553 M nitrous acid (HNO2) and 0.663 M of potassium nitrite…

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Q: Calculate the pH of a buffer solution prepared by dissolving 0.150 mol of benzoic acid and 0.300 mol…

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.