Calculate the pH of a 0.075-M  Al(NO3)3 solution. The Ka value for Al(H2O)63+ is 1.4x10 -5

Q: The pH of a 0.50 M solution of an acid, HA, is 4.67. Calculate Ka of HA.

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Q: The CO2 we breathe reacts with water in our blood to form the weak acid H2CO3. What mole ratio of…

A: Given:Ka of H2CO3 is 4.4 ✕ 10−8

Q: 8. Classify as spontaneous or no reaction. If spontaneous, write out the complete reaction. a) Ni²+…

A: Here we have to predict whether the following given redox reactions are spontaneous or not.

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: What is the pH of a 0.35 M solution of hydrofluoric acid with a Ka of 6.6 x 10-4? О 3.23 O 5.47 O…

A: Given: Concentration of HF = 0.35 M Ka of HF = 6.6x10-4

Q: what is the pH of a 0.11M solution of (CH3)3N, a weak base (Ka = 6.3 x 10^-5) ?

A: Given,Molarity of trimethyl amine , (CH3)3N = 0.11 MNote:   (CH3)3N is a weak base so Kb of  (CH3)3N…

Q: Calculate the pH of a solution that has an ammonium chloride concentration of 0.043 M and an ammonia…

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Q: Calculate the pH of a 0.25M aqueous solution of sodium fluoride, NaF. (Ka = 6.7 x 104)

A: Given; Concentration of sodium fluoride (NaF) solution = 0.25 M Ka = 6.7 × 10-4 pH of the solution =…

Q: Arsenate (AsO43) is highly toxic as it is incorporated instead of phosphate in many biomolecules.…

A: THE REMOVAL OF 1ST H+ IS SHOWN IN THE FOLLOWING REACTION, H3AsO4aq⇌H2AsO4-aq+H+aq THE ICE TABLE IS…

Q: Calculate the pH of a 0.500 M aqueous solution of HCOOH. ka = 1.77 x 10-4

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Q: Calculate the pH of a 0.40 M solution of benzoic acid, C6H5COOH? (Ka-6.3 x 10-5) What is the %…

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Q: Calculate the pH of a 5.3 x 10-3-M solution of H2S04 (Ka, = 1.2 x 10-2). pH =

A: Given-> Concentration of H2SO4 = 5.3 × 10-3 M

Q: Calculate the pH of a 4.80×10-1 M aqueous solution of sodium nitrite (NaNO2). (For nitrous acid,…

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Q: What is the pH of a 0.190 M C6H5CO2H M solution if the K₂ of C6H5CO2H is 6.5 x 10-5?

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Q: Nitrous Acid (HNO2) has a Ka value of 5.6x10–4. Calculate the pH of a solution that is 0.00298 M…

A: pH = -log[H+] For a weak acid solution: [H+] = (Ka x C)1/2 Where, C = molarity of acid

Q: What is the pH of a solution of 0.79 M acid and 0.55 M of its conjugate base if the ionization…

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Q: . Calculate the pH of a 0.0368 M aqueous solution of nitrous acid (HNO2, Ka = 4.5×10-4).

A: HNO2 is a weak acid and does not undergo complete dissociation in solution.

Q: Calculate the pH of a 0.063-M Al (NO3), solution. The K, value for Al (H2O),* is 1.4 x 10-º. pH =|

A: Given that: concentration of Al(NO3)3 = 0.063 M Ka = 1.4 ×10-5  To find: The pH?

Q: Phosphoric acid, H, PO,(aq), is a triprotic acid, meaning that one molecule of the acid has three…

A: A triprotic acid is an acid that has three dissociable protons. When such an acid undergoes stepwise…

Q: Calculate the pH of a 0.563 M solution of NaF. The Ka for the weak acid HF is 6.8 x 10-4. pH =

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Q: Propionic acid, HC3H5O2, has Ka= 1.34 x 10–5. (a) What is the molar concentration of H3O+ in 0.15 M…

A: HC3H5O2 is a weak acid and dissociates in aqueous solution as: HC3H5O2+H2O↔C3H5O2-+H3O+

Q: The following questions refer to a sodium hypochlorite (NaCIO) solution. HCIO K₂ =2.9 x 10-8 a)…

A: NaClO is a salt of weak acid and strong base. pH of this solution can be calculated by the following…

Q: Calculate the pH and the pOH of these solutions:   (c) 0.957 M HC2H3O2 (Ka = 1.8 x 10-5) pH =   pOH…

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Q: HCIO is a weak acid (Ka 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A: Given data; Ka=4×10-8Also, Kw=Ka×KbAnd,Kw=1×10-14 Consider the dissociation of given weak acid as;…

Q: Calculate the pH of a 0.355 M solution of propanoic acid, for which the Ka value is 1.30 x 10-5.

A: Given : concentration = 0.355 M               Ka = 1.30 × 10-5

Q: Let's assume that there is 400 μatm of pCO2 in our atmosphere. Assuming there is nothing else in the…

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Q: Calculate the pH of the solution that contains 0.145 M NH3 and 0.192 M NH4Cl.  The Ka of NH4+ is…

A: The solution will be the buffer solution if the weak acid and its corresponding conjugate base are…

Q: Explain what happens to the ratio of the two common forms of free residua! chlorine as the pH of…

A: Hypochlorous acid, HOCl(aq) is a weak acid with Ka = 2.5*10-8  Hypochlorite, ClO-(aq) is a conjugate…

Q: How many grams of lithium formate (LiCHO2) need to be dissolved in 184 mL of a 0.664 M formic acid…

A: Given: Concentration of HCHO2 i.e. the weak acid = 0.664 M Volume of solution = 184 mL = 0.184 L…

Q: How many grams of potassium lactate (C3H5O3K) need to be dissolved in 129 mL of a 1.71 M lactic acid…

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Q: In the laboratory, a general chemistry student measured the pH of a 0.590 M aqueous solution of…

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Q: What the pH of a solution containing [H3O+] = 5.62 x 10-11 mol L-1 ?

A: Given that, for a solution [H3O+] = 5.62×10-11 mol/L. We have to calculate the pH of the solution.

Q: HCl(aq) + H₂O(l) ⇒Cl¯(aq)+ H3O+ (aq) does water act as a Brønsted-Lowry acid, a Brønsted-Lowry base,…

A: we have to determine of water acts as Bronsted Lowry acid or base in the given reaction

Q: Calculate the pH of a 0.75 mol L─3 solution of ethanoic acid at 298 K. Given Ka = 1.7 × 10─5

A: Welcome to bartleby ! We have to calculate pH .

Q: Calculate the pH of each of the following buffered solutions. Ka (HC2H3O2) = 1.8 × 10-5 1. 0.11 M…

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Q: Please answer these questions on your Page 8 (a) 1 ) HA(aq) is a weak acid with a dissociation…

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Q: Calculate the pH of a 0.22 M codeine solution (Kb = 1.6ã10−6).

A: The value of Kb for the given weak base is = 1.6x10-6 The concentration of the base solution is =…

Q: If the Ka for Al3+ is 1.00x10-5, then what is the pH of 0.250M Al(NO3)3?

A: Step 1: Step 2: Step 3: Step 4:

Q: for h3po3, ka1 = 2.26 x 10-2 and ka2 = 4.79 x 10-7. calculate the ph of a 0.321 molar solution of…

A: Given,  for h3po3, ka1 = 2.26 x 10-2 and ka2 = 4.79 x 10-7. The ph of a 0.321 molar solution of…

Q: Muscles produce lactic acid, CH₂ CH(OH)COOH(aq), during exercise. Calculate the percent ionization…

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Q: The pH of an aqueous solution of 0.0319 M potassiumnitrite, KNO2, is This solution is (Assume that…

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Q: 3+ Calculate the pH of a 0.064-M Al (NO3); solution. The K, value for Al (H20)," is 1.4 x 10.

A: Concentration of Al ion = 0.064 M

Q: The pH of a 0.61 M aqueous solution of HNO2 (Ka = 4.6 × 10–4 at 298 K) is ____.

A:

Q: HCIO is a weak acid (K, = 4.0 x 10-) and so the salt NaCIO acts as a weak base. What is the pH of a…

A: HClO is a weak acid. NaClO is a salt made from strong base NaOH and weak acid HClO.  So, solution of…

Q: Calculate the pH of a 0.0449 M aqueous solution of nitrous acid (HNO2, Ka = 4.6×10-4) and the…

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Q: Calculate the pH of a 0.619 M solution of NaF. The Ka for the weak acid HF is 6.8 × 10-4.

A: Basic salt is the Salt formed from strong base and weak acid. solution 0.619 M NaF NaF is the Salt…