What is the OH- concentration in 0.5 M NH4Cl (aq)? (Ka of NH4+ = 5.6 X 10-10) A.) 5.6 × 10-10 M B.) 0.5 × 10-10 M C.) 1.7 × 10-5 M D.) 2.4 × 10-5 M

Q: 4. A weak acid, HX, has Ka = 7.9 x 10-5. Calculate [HX], [X-], [H+], and the pH of a 0.0380 mol/L…

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Q: A.Determine the [H+] , pH, and pOH of a solution with an [OH−] of 0.0087 M at 25 °C. [H+]= M pH=…

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Q: How many moles of HA would need to be added to 481 mL of 0.816 M NaA to produce a solution with a pH…

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Q: Determine the OH-, pH, and pOH of a solution with a H+ of 5.0 x 10-9 M at 25 °C. [OH"] = M pH РОН %3…

A: The acidity and alkalinity of a solution depends upon the concentration of hydronium ion and…

Q: Calculate the OH and the pH of a solution with an [H] = 5.6 x 10-¹0 M at 25 °C. [OH-] = 1.8 x10-5 pH…

A: The sum of the pH and pOH should be 14 always.  For multipart questions, we are asked to solve the…

Q: What is the pH of a 0.0015 M solution of HBr?     5.65     You need the Ka value to answer this…

A: What is the pH of a 0.0015 M solution of HBr?

Q: Calculate the pH of a HNO3 solution with a hydrogen ion concentration of .98M A. 0.00877 B 0.1 C…

A: Given, [HNO3] = 0.98M

Q: (a): [H3O+] = 1.0 x 10-5 M at 25°C: what is the OH−concentration?  Is the solution acidic, basic,…

A: Since you have posted multiple questions, as per our company guidelines we are supposed to answer…

Q: Calculate the [H +] in a solution that has a pH of 8.55.

A: Equation for pH calculation is:

Q: Determine the [OH−] , pH, and pOH of a solution with a [H+] of 2.7×10−9 M at 25 °C. [OH−]= pH= pOH=…

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Q: At 25°C, what are the molar H3O+ and OH- concentrations in a. 0.200 M NaOCI? b. 0.0860 M…

A: Since you have asked a question with multiple subparts, we will answer only first three subparts for…

Q: The pH of 0.259 M solution of an unknown acid is measured to be 2.353. What is the Ka of the acid?

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Q: Calculate [OH-] and pH of the following solutions. a. A 0.225 M solution in KOH. b. A 0.0015 M…

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Q: A solution of washing soda (sodium carbonate, Na2CO3) has a hydroxide ion concentration of 0.0040…

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Q: Lab 6 A solution has (OH concentration equal to 4.78 x 10 1 What is the pH? Please put answer in box…

A: Answer

Q: a. Determine the [OH−][OH−] , pH, and pOH of a solution with a [H+][H+] of 8.8×10−9 M8.8×10−9 M at…

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Q: The weak acid HQ has a pKₐ of 4.89.(a) Calculate the [H3O⁺] of 3.5X10⁻² M HQ.(b) Calculate the…

A: Calculation of dissociation constant:

Q: Find the values of [H'], pOH, [], that correspond to each of the following lues: [H'] [OH] РОН pH of…

A: The question is based on the concept of PH and pOH calculations.   pH is defined as negative…

Q: What is pH of a solution consisting of 1.05 M NH3 and 0.98 M NH4NO3? Ka of NH4 + is 5.8 x 10-10…

A: 1.05 M NH3 and 0.98 M NH4NO3 The NH4NO3 dissociate as ; NH4NO3 =  NH4+  + NO3-  So the Concentration…

Q: Q1/ Calculate the concentrations of the an ions species in (0.1 M H₂ASO4): [H], [OH'], [H₂AsO4].…

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Q: Formic acid, HCOOH, is a weak acid with a Ka equal to 1.8×10 –4.  What is the pH of a 0.115 M…

A: Given: Ka is 1.8×10 –4 Molarity of formic acid is 0.115 M. Introduction: A weak acid dissociates…

Q: What is the pH of a solution that has an initial HA concentration of 0.93 M, with a Ka = 1.4 x 10-7?…

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Q: Calculating the PH UI A solution is prepared at 25 °C that is initially 0.45M in ammonia (NH,), a…

A: Initial concentration of ammonia=0.45M  Concentration of ammonium chloride=0.13M  Kb=1.8×10^-5 pH of…

Q: What is the pH of a solution with [H+]=2.2 x 10-7  M? a. pH = 7.3 b. pH = 5.7 c. pH = 2.2 d. pH =…

A: Which one of the following is correct answer

Q: ich of the following is usually considered to be a weak acid? A) HCI B) HBr C) HI D) HF CH 26. Which…

A: (25) Given acids are  HCl, HBr, HI, HF    Among these acids HF is considered as a weak acid because…

Q: Formic acid, HCOOH, is a weak acid with a Ka equal to 1.8×10–4.  What is the pH of a 0.0115 M…

A: Introduction : Formic acid is a colourless , fuming liquid with a pungent smell with the chemical…

Q: The pH of a 8.3×10-2-M solution of phthalic acid (H2C8H4O4) is measured to be 2.03. Use this…

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Q: What is the pH of a 0.150 M NH4Cl solution? Kb of NH3 = 1.76 × 10−5

A: Given: Concentration of NH4Cl = 0.150 M Kb for NH3 = 1.76×10−5

Q: Rank the acidity from most to least for given solutions. I. a solution with [H3O+] = 4.2 × 10−6 M…

A: More the H+ ion more will be the acidic nature. Lower the pH of solution greater will be the…

Q: What is the pH of a 5.58×10-5 M solution of the strong acid HCl? HCl(aq) + H2O(ℓ) → Cl-(aq) +…

A: The pH of the two solution has to be determined. The formula to calculate the pH is,…

Q: Anisic acid (Ka=3.38x10^-5) is found in anise seeds and is used as a favoring agent. For a 0.867 M…

A: From given concentration of anisic acid = 0.867 M  So from that  All given categories like  H+, OH-,…

Q: Determine the [OH−], pH, and pOH of a solution with a [H+] 7.7×10^−11 M at 25 °C [OH−]=     pH=…

A: Since,           At 25°C[H+] [OH-] =10-14PH+POH=14PH = -log [H+]POH=-log  [OH-]

Q: What is the pH of a 0.300 M NH3 solution that has Kb = 1.8 × 10-5? The equation for the dissociation…

A: We have given the balance chemical equation                                      NH3(aq)     +…

Q: For the diprotic weak acid H2A, Ka1 = 3.1 × 10-6 and K2 = 8.4 × 10-9. What is the pH of a 0.0500 M…

A: The concentration of diprotic weak acid H-A is 0.0500 M. The value of acid dissociation constant Ka1…

Q: Determine the [OH−], pH, and pOH of a solution with an [H+] of 2.4×10−13 M at 25 °C. [OH−]= pH= pOH=

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Q: Calculate the [OH-], pH and percent ionization for a 0.20 M aqueous NH3 solution.          NH3 + H2O…

A: The Kb is the equilibrium constant for the reaction of the base ammonia combining with water to…

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: H2CO3 is weak diprotic acid so its pH is not directly calculated

Q: Determine the [OH−] , pH, and pOH of a solution with a [H+] of 5.7 ×10−11 M at 25 °C. [OH−]= M pH=…

A: For 1st:Given:[H+]  = 5.7 x 10-11 Mwe have to find:[OH-] =??pH= ??pOH =??

Q: A student needs a sample of 0.772539887245 M NaOH for a laboratory experiment. Calculate (a) the…

A: It is given that the concentration of sodium hydroxide (NaOH) sample is 0.772539887245 M, the…

Q: 1. How much base 0.1 M NaOH was required to neutralize lemon juice from our experiment part 1, and…

A: Solution :      pH       pH is a quantitative measure for the acidity or basicity of the solution.…

Q: 200 g of phosphoric acid (H3PO4) is dissolved into 10 L of water. pKa1=1.3, pKa2=7.21, pKa3=12.32.…

A: Phosphoric acid , H3PO4(aq) is a triprotic acid that can donate up to 3 protons.  The Ka values are:…

Q: Determine the pH of the solution to the correct number of significant figures.

A: We have to find the pH of solution

Q: HIO3 has a ka of  0.16. What is the pH of a 0.600 M HIO3 solution? (use successive approximations)

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Q: f the following salts are each dissolved in water to form 0.1 M solutions at 25 °C, which will have…

A: given solutions ;  1) NOCl  2) KCl 3) NH4Cl 4)Ca(CH3COO)2

Q: What is the percent ionization of 7.5x10-2 M HCN?  Ka =  4.0 x 10-10  for  HCN.

A: Given, Concentration of HCN (C) = 7.5 × 10-2 M Ka for HCN = 4.0 × 10-10 Percent ionization = ?

Q: Find the pH of each mixture of acids. a) 7.5×10−2 M in HNO3 and 0.175 M in HC7H5O2 b) 1.5×10−2 M in…

A: a) The hydrogen concentration of nitric acid and benzoic acid are calculated as,

Q: Calculate [H+] in a solution that has a pH of 9.77. a. 5.9*10^9 b. 1.7*10^-10 c. 5.9*10^-9 d.…

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Q: the blood has a pH of 7.53 and has 22 mmol/L bicarbonate ion concentration, what is the molar…

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Q: Calculate the pH for a 7.32×10^−6 NH3 solution with a Kb=1.76 * 10^-5 . NH3(aq) + H2O (l)…

A: To find pH

Q: What is the pH of 0.1510 M selenious acid solution, H2SeO3? H2SeO3(aq) + H2O(l) → HSeO3−(aq) +…

A: As the second ionization constant Ka2 is very less than first ionization constant Ka1, the Ka2 can…