Q: Find the mass of sodium formate that must be dissolved in 250.0 cm3 of a 1.4 M solution of formic…
A:
Q: What is the pH of a buffer solution containing 0.21 M HNO2 and 0.10 M NO, ?
A: Since HNO2 is a weak monoprotic acid with pKa = 3.15 And the solution is given buffer solution with…
Q: calculate the buffer capacity of a buffer consisiting 0.05 moles each of acetic acid and sodium…
A:
Q: A volume of 40.0 mL of 0.100 M CH3COSH (aq) is titrated with 0.100 M NaOH(aq). What is the pH after…
A:
Q: A buffer solution is 0.320 M in H3PO4 and 0.254 M in KH2PO4. If Kal for H3PO4 is 7.5 × 10-3, what is…
A: H3PO4 is acid and KH2PO4 is a conjugate base of this acid. We use the Henderson Hasselbalch equation…
Q: A solution was found to have a PH of 6.3 with the acid 100x in excess of it conjugate base. What is…
A: According to Henderson-Hasselbalch equation,pH = pKa + log [conjugate base/acid]
Q: Which of the following accurately describes the major species in solution at point C on the…
A:
Q: Explain what chemistry occurs in each region of the titration of the weak base, A, with strong…
A: pH - pH is defined as negative logarithm to the base 10 of H+ ion concentration. pH value determines…
Q: A 50.00 mL aliquot of 0.0100 M NH3 is titrated with 0.02136 M HCl. What is the pH of the solution at…
A:
Q: Why is titrant added rapidly at the beginning of titration but more slowly as titration proceeds?
A: At the beginning, the amount of analyte present in the solution will be high. Hence whatever amount…
Q: A 34.9 mL sample of a 0.423 M aqueous hypochlorous acid solution is titrated with a 0.474 M aqueous…
A:
Q: A buffer solution is 0.396 M in HF and 0.233 M in KF. If Ka for HF is 7.2x10-4, what is the pH of…
A:
Q: What volume of 0.2M HCI must be added to 250ml of 0.3M sodium mandelate to produce a buffer solution…
A: Given, Molarity of HCl = 0.2 M Molarity of sodium mandelate (say NaA) = 0.3 M Volume of sodium…
Q: The titration of a weak monoprotic acid by NaOH is shown here. The optimal buffering capacity of…
A: The titration curve given is,
Q: 1. A 25.00 mL solution of 0.0920 M HNO3 was titrated with 0.00, 15.00, 23.00, and 30.00 mL of 0.1000…
A: The titration reaction will be as follows: HNO3 + KOH ------------> KNO3 + HOH. The volume of…
Q: A buffer solution is prepared by dissolving 1.300 g of ammonium chloride (NH4Cl) into 100.00 mL…
A: Mass of ammonium chloride is 1.3 g. Molar mass of ammonium chloride is 53.491 g/mol.
Q: A buffer solution is 0.438 M in HNO2 and 0.236 M in KNO2. If Ka for HNO2 is 4.5x10-4, what is the pH…
A: Given: concentration of HNO2 = 0.438 M concentration of KNO2 = 0.236 M Ka for HNO2 = 4.5 × 10-4…
Q: 1.Calculate the pH and the of a buffer made from 0.28 M HNO₂ and 0.23 M NO₂. (The Ka for HNO2 is 4.6…
A: Given, Ka(HNO2) = 4.6×10-4
Q: Calculate the pH at the equivalence point of a titration of 0.3326 g of THAM (pKa of conjugate base…
A: Calculation of molarity of THAM from molar mass:
Q: A buffer solution is prepared by dissolving 1.000 g of ammonium chloride (NH,CI) into 100.00 mL of a…
A:
Q: 3) Arsenic acid has 3 pK,'s: 2.19, 6.94, and 11.51. Determine the concentrations of all the species…
A: Since you have asked multiple questions, we will solve the first one for you. For remaining…
Q: Which of the following 1:1 mixtures would be best suited to form a buffer closest to a pH of 3.70?
A: In order to prepare a buffer closest to a pH value of 3.70, the buffering range of the resulting…
Q: What is the pH at the equivalence point when 0.10 M HNO3 is usedto titrate a volume of solution…
A: A quantitative measure of the acidity or basicity of aqueous solutions. Equivalence point in a…
Q: Calculate the pH of a buffer solution obtained by dissolving 0.1 moles of pyridine (C5H5N) and 0.2…
A: Number of moles of pyridine = 0.1 moles Number of moles of pyridinium chloride = 0.2 moles
Q: A sodium hydrogen carbonate-sodium carbonate buffer with a pH of 9.40 is prepared. Determine the…
A: Given: The pH of the sodium hydrogen carbonate-sodium carbonate buffer = 9.40 We have to find the…
Q: 2. There is a phosphate buffer with 0.1 M of NaH₂PO4 0.1 M of Na₂HPO4. Calculate pH of buffer…
A: A buffer solution is a combination of two solutions - a weak acid solution and the salt of its…
Q: What is the pH of a buffer solution containing 0.45M H3PO4 and 0.25M H2PO4- ?
A:
Q: A buffer solution is 0.405 M in HF and 0.200 M in KF. If Ka for HF is 7.2×10-4, what is the pH of…
A: Here given, Concentration of HF = 0.405 M Concentration of KF = 0.2 M Ka for HF = 7.2 x 10-4 We…
Q: 0.1 MHCI buffer solution with pH =7 0.1 MNAOH
A: The pH of a solution depends upon the concentration of the hydrogen ions.pH=-log10H+pH+pOH=14
Q: A buffer composed of 0.1 M CH3COOH/1.0 M CH3COO- has a lower buffering capacity as opposed to a…
A: We know that, buffer capacity range from ( pKa + 1 ) to ( pKa - 1 ) Buffer capacity very less at…
Q: 2. There is a phosphate buffer with 0.1 M of NaH2PO4 0.1 M of Na2HPO4. Calculate pH of buffer…
A: pH of a buffer solution can be calculated using H-H equation.
Q: Which hydroxide has the lowest molar solubility in H2O?
A: Ksp is know as the solubility product constant. The above mentioned question is explained below :
Q: What is the pH at the equivalence point in the titration of 0.50 M KOH with 1.00 L of 0.750 M HF(aq)…
A: 1- First calculate the volume of KOH : We will used the equation, ( M2V2)KOH = ( M1V1)HF ( 0.50M ×…
Q: Calculate the pH at the equivalence point for the titration of 0.100 M methylamine (CH, NH,) with…
A:
Q: What is the primary species in solution at the halfway point in a titration of NH: with HBr? A) NH:…
A: Ammonia is highly soluble in water. Ammonia reacts with water to form ammonium hydroxide. NH3aq +…
Q: Calculate the ph of at second equivalence point when 0.10M trisodium arsenate is titrated with 0.20…
A: trisodium arsenate, Na3AsO4(aq) is a deprotonated form of H3AsO4(aq), which is a tribasic acid. The…
Q: what is the ph at equivalance point in the titration of 100ml of 0.20M of ammonia with 0.10M of…
A: Given :
Q: Calculate the pH of the following buffers:a) A solution containing 0.425 molar benzoic acid and…
A: Calculate the value of pKa: Ka of benzoic acid is 6.50 × 10-5.
Q: A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in LiF. Calculate the pH of the solution after…
A: The equation is given below,HF(aq) + LiOH(aq) → LiF(aq)+H2O(l)
Q: The pOH of an acidic buffer is 9.725. What is the Ka of the acid if the ratio of [ionized] to…
A: pOH = 9.725 Ratio = 1380
Q: A student has a sea water sample which contains Ca2 ions . Describe briefly how he will determine…
A: To determine the concentration of calcium ions, we have to perform titration with EDTA solution. In…
Q: 5. What is the "equivalence point" of a titration?
A: Titration is a laboratory method used to determine the unknown concentration of acid or base. The…
Q: How is the equivalence point determined in potentiometric titrations? Please explain briefly.
A: Answer is explained below.
Q: what is the pH of this buffer solution?
A: Given :- concentration of HNO2 = 0.309 M concentration of NaNO2 = 0.340 M Ka = 4.5 × 10-4 To…
Q: Describe the shape of the titration curve shown, describe why it has this shape.
A: Titration between strong acid - strong base gives rise to S-shaped titration curve.
Q: A buffer solution is 0.397 M in H2S and 0.382 M in KHS. If Kaj for H2S is 1.0 × 10-7. what is the pH…
A:
Q: When determining water by the K method. Fisher's end point of titration is determined by Choose one…
A: The Kark-Fisher titartion is used to determine the amount of water in a sample. The principle of…
Q: The titration of 50.0mL ot HC2H3O2 (Ka=1.8 x 10-5) 0.100M NAOH. The pH of solution at the Equivalenc…
A:
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- Titration of 50.00 mL of 0.04715 M Na2C2O4 required 39.25 mL of a potassium permanganate solution. 2MnO4- + 5C2O4-2 +16H+ -> 2Mn2+ + 10CO2(g) + 8H2O Calculate the molar concentration of the KMnO4 solution What molecules would interfere with the titrimetric analysis?25mL of saturated KHC4H4O6 was prepared and titrated with 6.91mL of 0.0250M NaOH.a. What is the Ksp and molar solubility of KHC4H4O6?b. If KHC4H4O6 is dissolved in 25mL of 0.1M KCl, how much 0.0250 M NaOH will be used?At 25ºC, AgCl (Ksp = 1.6 x 10-10) is less soluble as compared to PbCl2(Ksp = 2.4 x 10-4) True or false?
- A new indicator was found, at pH values less than 7.5 the indicator is blue and at values greater than 9.5 itis grey.A) What is the approximate pKa for this indicator?B) At a pH of 5.0, which species is dominant? HIn or In-?C) At a pH of 7.5, which species is dominant? HIn or In-?D) At a pH of 10.0 which species is dominant? HIn or In-?A 25.00 mL solution was prepared by dissolving CaCO3 solid. It required 24.25 mL of a standard 0.02 M EDTA (ethylenediaminetetraacetic acid) solution to titrate the Ca2+ ions to the end point. (moles= 4.85 * 10^-4) a. How many moles of EDTA are contained in the 24.25 mL used for tritration. b. How many moles of CaCO3 were used? c. What is the concentration (molarity) of Ca2+ in the 25.00 mL of solution?A Fajans titration of a 0.7908-g sample required 45.32 mL of 0.1046 M AgNO3 . Express the results of this analysis in terms of the percentage of BaCl2 * H2O. (Use a MW value in 4 decimal places)
- 1. The molar solubility of Ag2SO3 is 1.55× 10-4 M. Calculate the Ksp of Ag2SO3. a. 7.45 x 10^-12 b. 1.55 x 10^-4 c. 2.40 x 10^-8 d. 1.49 x 10^-11 e. 3.72 x 10^-12 2. What is the difference between the end point of an acid–base titration and the equivalence point? a. There is no difference; these are just two terms meaning the same thing. b. At the end point, the acid and base are present in equal numbers of moles. At the equivalence point, the indicator changes color. c. The end point is always at pH 7 but the equivalence point can be at various pH values. d.The end point can be at various pH values but the equivalence is point always at pH 7. e. At the end point, the indicator changes color. At the equivalence point, the acid and base are present in equal numbers of moles A solution at 25 °C that contains 1× 10-8 M H3O+ is a. basic b. acidic c. neutral d. both acidic and basicA solution containing Mg2+ was buffered to pH 9.81 and titrated with EDTA. Eriochrome black T, with p?a1 = 6.3 and p?a2 = 11.6 was used as the indicator. It is a diprotic acid, H2E What is the fraction of the predominant form of eriochrome black T in solution at this pH? (To answer this, report the alpha fraction of the indicator’s most prevalent species at this pH)The Kjedahl procedure was used to analyze 256 µL of a solution containing 37.0 mg protein/mL. The liberated NH3 was collected in 5.00 mL of 0.033 6 M HCl, and the remaining acid required 6.34 mL of 0.010 M NaOH for complete titration. What is the weight percent of nitrogen in the protein? wt%
- Consider a titration of 40.00 mL of 0.1250 M Na2CO3 with 0.4000 M HCl. Carbonic acid (H2CO3) has a pKa1 of 6.351 and a pKa2 of 10.329. What is the pH at the second equivalence point?1.) The solubility product, Ksp, of Cd3(PO4)2 is 2.5 x 10-33. What is the solubility (in g/L) of Cd3(PO4)2 in pure water? 2.) The solubility product of Cu(OH)2 is 4.8 x 10-20. Calculate the value of pCu2+, or -log[Cu2+], in an aqueous solution of NaOH which has a pH of 12.45 and is saturated in Cu(OH)2. 3.) The equilibrium constant for the formation of Cu(CN)42- is 2.0 x 1030. Calculate the value of pCu2+, or -log[Cu2+], if we were to dissolve 2.52 g of CuCl2 in 1.000 L of a solution 0.946 M in NaCN. The addition of CuCl2 does not alter the volume (the final volume is still 1.000 L).The B4O5(OH)4^2- ion, present in 5.0 mL of a saturated Na2B4O5(OH)4 solution at a measured temperature, is titrated to the bromoscresol green endpoint with 5.25 mL of 0.182 M HCL. What is the Ksp for Na2B4O5(OH)4?