Assume each salt below is dissolved in water to make a 1M solution. Chose if that solution is acidic, basic, neutral, or you would need more information to make that determination. • (CH3)3NHF [ Select] • NaHSO4 Acidic • Na2SO4 [Select] • Ca(CO3)2 [Ca(CO3)2] • C5H5NHBr Acidic

Q: Which of the following statements is TRUE? Select one: O a. FT cannot act as a Bronsted-Lowry base,…

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Q: pKa НА 5.34 HB 3.22 HA + B = A + HB A) There should be more products at equilibrium because HA is a…

A: Applying concept of Pka and acid strength relationship.

Q: A solution is prepared by dissolving 4.50 g of solid NaOH in 1.00 L o 0.100 M HNO₂(aq) (Ka =…

A: The pH of the solution can be calculated as follows

Q: 1. The oxalate ion concentration, C;0. of 0.20 M H;C0 is adjusted to a value of 3.00 x 10 M. What is…

A: As per the guideline, since you have asked multiple questions, we have solved the first question for…

Q: For H2CO3, Ka1 = 4.3 × 10–7, Ka2 = 4.7 × 10–11. What is the pH of a 0.36 M solution of carbonic…

A: We have to predict the pH of 0.36 M of carbonic acid .

Q: Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH…

A: Given,  Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. The pH…

Q: Rank the following salts in order of increasing pH of their 0.1 M aqueous solutions:(a) KNO3, K2SO3,…

A: a) The given salts are The concentration of the solution is given as 0.1M

Q: Use the media upload button to show your work. %3D Determine the K, of an acid when 0.2005 M of this…

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Q: John made a buffer solution A at pH =8, and pKa = 9.

A: Given: Buffer solution A have pH= 8 pKa = 9 To determine: The buffer solution A have more buffer…

Q: A student performs a spot test to identify the ions in an unknown solution. The student did a series…

A: Test for phosphate (PO43-) Addition of aqueous (NH4)2MoO4 to an aqueous solution containing PO43-…

Q: Which of the following is an acidic salt? O a. Na2SO4 O b. NaCI С. КС O d. NH4CI O e. CH3COONa

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Q: Consider the following compound: [Cr(en)2(H20)]SO4. Which of the following is the Lewis acid? O H20…

A: Answer - Lewis acid - A Lewis acid is therefore any substance, such as the H+ ion, that can accept a…

Q: Consider the following oxides: Cro, Cr203, CrOz. Which is most acidic? 2 Edit SHOW HINT (b) Which is…

A: The oxidation number of Cr in CrO = +2 The oxidation number of Cr in Cr2O3 = +3 The oxidation number…

Q: What is the pH of a solution that is 0.0032 M in HA and also 0.087 M in NaA? (Ka = 4.1 × 10-6) 6.56…

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Q: 2H3O2 HO2 Ka = 1.8E-4 %3D

A: acidic strength increase as the releasing power of H+ increase. HBr is more acidic because size of…

Q: 23.) Which of the following species is amphoteric? A) CO, 2- B) HF C) NH,* D) H;PO, E) None of the…

A: Amphoteric species: It is defined as the species that can acts as both an acid and a base. Or,…

Q: Calculate the Ka of a 0.50 M HC4H7O2 with a pH of 2.56

A: The concept used here is based on the acid dissociation constant of an acid which is used for…

Q: Be sure to answer all parts. The uses of sodium phosphate include clarifying crude sugar,…

A: Given that   Ka3 = 4.2× 10^-13

Q: An aqueous solution of sodium ethanoate is alkaline having a pH value greater than 7 46. Sodium…

A: 46.  First statement is sodium ethanoate is alkaline having pH greater than 7.  Sodium ethanoate +…

Q: What is the pH of a solution that is 0.063 M in HA and also 0.023 Min NaA? (Ka = 4.1 × 10- O. 5.46…

A: Given: The concentration of HA is 0.063 M The concentration of NaA is 0.023 M The Ka value is 4.1 x…

Q: Calculate the concentration of all species in a 0.470 M solution of H2SO3. The acid ionization…

A: The H2SO3 solution contains the following species,

Q: What volume of 0.1543 M NaOH must be added to 25.00 mL of 0.2405 M HCOOH in order to prepare a…

A: Ka = 1.8 ×10–4 pKa = – logKa = – log(1.8 ×10–4) = 3.745 Let n be the number of millimoles of NaOH to…

Q: Calculate the concentrations of HF, OH−, and H3O+ in a 0.19 M KF solution (for which…

A: Given: The concentration of KF solution = 0.19 M Ka for HF = 6.8 × 10-4 We have to calculate the…

Q: Determine [OH−], pH, and pOH of a 0.25 MM ammonia solution. For NH3, Kb=1.76×10−5.

A: The question is based on the concept of equilibrium. ammonia is a weak base. so, partially…

Q: Write a balanced chemical equation for the reaction occurring when CH3CH2COOH is added to water.…

A: Write a balanced chemical equation for the reaction occurring when CH3CH2COOH is added to water.…

Q: this question. Calculate the pH of a solution that is prepared by dissolving 0.168 mol of…

A: The two given acids dissociate partially as- C6F5COOH→C6F5COO- + H+      Ka= 3.30×10-2HClO →H+ +…

Q: Which of the following are/is a physical property of an acid? a. low pH Value b. High pH value c.…

A: Answer Physical property of acid The pH range goes to 0 to 14…

Q: Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH…

A: Given : Concentration of H2CO3 = 0.33 M Ka1 of H2CO3 = 4.3 X 10-7  And Ka2 of H2CO3 = 5.6 X 10-11…

Q: What is the pH of a 0.618 M carbonic acid (H2CO3) solution given Ka1=4.4×10−7 and Ka2=4.7×10−11?

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Q: Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH…

A: The carbonic acid is a diprotic acid. The major release of hydrogen ions occurs in the primary…

Q: A basic solution turns , litmus paper to Select one: O Blue: Red O Red; Red O Blue: Violet Red; Blue

A: Bases are the substances that produce OH- ions when dissolved in water. The litmus test helps to…

Q: Part II. Arrange the following compounds in order of increasing basicity. 7. NazO, Rb2O, K2O 8.…

A: Ans. Part II Arrangement of the given compounds in order of increasing basicity: (7)  Na2O <…

Q: Which of the following salts would produce the most acidic 0.10 M aqueous solution? FeCl, KF, KNO,…

A: FeCl is the right answer. Whichever is the stronger acid will be the dominate factor in determining…

Q: The salt resulting from the reaction of HNO, with NH3 would have an acidic characteristics. Select…

A: Salt hydrolysis :   It is a type of reaction in which one of the ions from the salt reacts with…

Q: 1. Calculate the pH of 0.10 M (COOH)2 (aq), oxalic acid. Ka1 = 5.9 × 10–2 ; Ka2 = 6.4 × 10–5.

A: Note - Since you have asked multiple question, we will solve the first question for you. If you…

Q: Nahso3 titr. In neutral describe how the color goes from Mn04- to MnO2 In basic w NaOH describe…

A: Answer-1 In neutral medium, SO32- ion of NaHSO3 is oxidized by MnO4- ion into sulfate ion and MnO4-…

Q: A buffer solution is 0.357 M in H2 C204 and 0.399 M in NaHC204. If Kal for H2 C204 is 5.9 x 10-2,…

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Q: Given the following compounds: H2S (34.065); NaHS (56.065); Na,s (78.065), calculate the pH of a…

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Q: Calculate the pH of a solution resulting from the addition of 50.0 mL of 0.30M HNO3 to 50.0 mL of…

A: Nitric acid which is a strong acid on undergoing a reaction with ammonia will form a salt of…

Q: 22:b) Solution A has a PH = 8.94 and Solution B has a [OH] = 4.5 x 10+ M. Which solution is more…

A: Here is the solution

Q: Calculate the sodium acetate/acetic acid ratio to prepare a buffered solution with a pH of 5.06.…

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Q: Indicate the type of oxide (acidic, basic or amphoteric) that best describes each of the following…

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Q: Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH…

A: Since the Ka1 of H2CO3 is >> Ka2 of H2CO3  Hence we can assume only the first dissociation of…

Q: Concentration: 0.50 M Buffer Solution: Phosphate pKa: 2.12 Desired pH: 3.0

A: Solution - According to the question - Given - we use Henderson Hasselbach equation, pH = pKa + log…

Q: Which of the following salts will form acidic solutions in water? Fe(NO3)3, LiClO4, Na3PO4, CrCl3,…

A: The nature of the salt will depend on the acid and base from which they have formed.  1 ) If they…

Q: Calculate the concentration of each species of oxalic acid in a 0.150 M solution of sodium oxalate,…

A:

Q: Calculate the pH of a 0.294 M NaF solution. Assume KA(HF) = 1.0 x 10-4 .  Give you answer to three…

A: Given : Concentration of NaF = 0.294 M Since NaF contains the ion F- which is conjugate base of weak…

Q: For a saturated solution of anunknown metal hydroxide (M(OH)2),13.75 mL of this solutionwere…

A: We will calculate the Kspof the    metalhydroxide.

Q: Show the calculations to demonstrate that 2% AgNO3 is approximately 0.1M in Ag+ ions.

A: Given:the given concentration of AgNO3 must be in w/vconcentration of AgNo3 (w/v)=2%The formula for…

Q: Rank the following in order of least-to-most acidic: B Br HO, HO, HO, Cl HO CI Br OC<B<A<D OD<A<B< C…

A: We have to arrange them in order of least to most acidic.