# In a 1.0x10^-4 M solution of HClO (aq), identify the relative molar amounts of these species.

## Question:

In a 1.0x10^-4 M solution of HClO (aq), identify the relative molar amounts of these species.

## Molarity

This is a measure of the concentration of a chemical species, in particular of a solute in a solution, in terms of the amount of substance per unit volume of solution. The units of molar concentration are moles per liter.

## Answer and Explanation: 1

Become a Study.com member to unlock this answer! Create your account

View this answerHClO is a weak acid, will not dissociate 100%

then

{eq}HClO + H_2O = H_3O^+ + ClO^- {/eq} {eq}K_a {/eq} < 1

{eq}H_3O^+ > OH^- {/eq}

{eq}H...

See full answer below.

#### Ask a question

Our experts can answer your tough homework and study questions.

Ask a question Ask a question#### Search Answers

#### Learn more about this topic:

from

Chapter 8 / Lesson 4What is molarity? What is molality? Compare molarity vs molality by viewing molality and molarity formulas, how to calculate molarity and molality, and examples.

#### Related to this Question

- In a 1.0 times 10^{-4} M solution of HClO(aq), identify the relative molar amounts of these species: HClO, OH^-, H_3O^+, OCl^-, H_2O.
- 1. A solution is labeled "0.671 M HClO." What are the following in the solution? Express your answers to three significant figures even when only two are valid. [ HClO]= [H3O+]= [ClO-]= pH= 2. Cal
- Determine the \begin{bmatrix}H_3O^+\end{bmatrix} in a 0.265 M HClO solution. The K_a of HClO is 2.9 \times 10^{-8}.
- Determine the H3O+ in a 0.315 M HClO solution. The Ka of HClO is 2.9 x 10-8.
- Determine the (H3O+) of a 0.265 M HClO solution. (Ka of HClO = 2.9 x 10-8)
- Determine the H3O+ in a 0.278 M HClO solution. The Ka of HClO is 2.9 x 10-8.
- HClO has a pKa of 7.54. What is the ClO- in a 0.110 M HClO solution?
- A solution of HClO is mixed and found to have a pH of 4.53. Find what the initial concentration of HClO was for this solution. Ka = 3.00 x 10^{-8} for HClO.
- HClO has a pKa of 7.54. What is the H3O+ in a 0.110 M HClO solution?
- Calculate the H3O+ in a 0.285 M HClO solution. (Ka = 2.9 x 10-8)
- Compute the percent dissociation of (a) 1.0 M HClO (b) 1.0 x 10^-4 M HClO.
- What is the (H3O+) of a 0.100 M solution of HClO? HClO has a Ka = 2.9 x 10-8.
- A solution of HClO is mixed and found to have a ph of 4.34. Find what the initial concentration of HClO was for this solution. Ka = 3.00 times 10^ -8
- Determine the percent ionization of a 0.014 M solution of hypochlorous acid, HClO. The Ka for the acid is 3.5 * 10^-8. A) 3.5 * 10 ^-6 % B) 4.9 * 10^-9 % C) 7.0 * 10^-3 % D) 5.0 * 10^-2 % E) 1.5
- The pH of a solution of hypochlorous acid, HClO, was measured to be 3.89. Calculate the molarity of this solution. The K_a for HClO is 3.0 times 10^{-8}.
- Find the percent ionization of a 0.287 M HClO solution. (The value of Ka for HClO is 2.9 x 10^-8.) Express your answer using two significant figures.
- The Ka of hypochlorous acid (HClO) is 3.00 x 10-8. What is the pH of a 0.0200 M HClO solution?
- Calculate the Ka for a 0.10 M HClO solution that is found to have a pH of 4.23.
- Determine the percent dissociation of a 0.17 M solution of hypochlorous acid, HClO. The Ka for the acid is 3.5 x 10-8.
- HClO has a pKa of 7.54. What is the pH of a 0.110 M HClO solution?
- Hypochlorous acid has a pKa of 7.54. What is ClO- in a 0.115 M HClO solution?
- Find the percent ionization of a 0.139 M HClO solution. (The value of K_a for HClO is 2.9 times 10^{-8}.)
- Calculate the pH of a 0.315 M HClO solution. (Ka = 2.9 x 10-8)
- Calculate the pH of a 0.285 M HClO solution. (Ka = 2.9 x 10-8)
- Solve for the pH of a solution that has 0.100 M HClO and 0.075 M NaClO. The Ka (HClO) = 2.9 x 10^{-8}.
- Determine the pH of a 0.278 M HClO solution. (Ka = 2.9 x 10-8)
- You have 1.0 liter of 0.45 M HClO (aq). At 25^oC, K_a = 3.5 \times 10^8 for this acid. Calculate the pH of 0.45 M HClO and the concentration of ClO^- at equilibrium.
- Calculate the pH of a 0.11 M hypochlorous acid (HClO) solution. (Ka = 4.0 x 10-8)
- A solution is prepared by adding 0.300 moles of hypochlorous acid (HClO) to enough water to make 1.00 L of solution. The K_a of hypochlorous acid is 3.5 times 10^{-8}. What is the concentration of [H^+] at equilibrium?
- Find the pH of an aqueous solution that is 0.0500 M in HClO. (Ka = 2.8 x 10-8)
- What is the pH of 35.1 mL of a solution that is 0.51 M in LiClO and 0.53 M in HClO? (For HClO, Ka = 3.5 x 10-8.)
- What is the H3O+ of a 0.35 M solution of HClO? (Ka = 2.9 x 10-8)
- What is the H3O+ of a 0.95 M solution of HClO? (Ka = 2.9 x 10-8)
- The acid-dissociation constant at 25.0 degrees C for hypochlorous acid (HClO) is 3.0 \times 10^{-8}. At equilibrium, the molarity of H_3O^+ in a 0.033 M solution of HClO is __________.
- Calculate the (OCl-) of a 7.03 x 10-2 M solution of the weak acid HClO (make an approximate calculation assuming that initial concentration is equal to the equilibrium concentration). Round your answer to 3 significant digits.
- Calculate the percent ionization of hypochlorous acid (HClO) in solution of each of the following concentrations (K_a= 3 e^{-08}). (a) 0.271 M (b) 0.302 M (c) 0.785 M
- What is the H3O concentration of a solution at equilibrium if it was prepared from 0.35 M hypochlorous acid, HClO, which has Ka = 4.0 x 10-8?
- Find the ClO- concentration for a mixture of 0.100 M HF in 0.150 M HClO Please show steps
- Determine the [H3O^+] in a 0.265 M HCIO solution. The Ka of HClO is 2.9 times 10^-8. A. 1.1 times 10^-10 M B. 7.7 times 10^-9 M C. 4.9 times 10^-4 M D. 1.3 times 10^-6 M E. 8.8 times 10^-5 M
- Calculate the pH of a buffer that is 0.85 M in HClO and 0.25 M in NaClO. The Ka for HClO is 2.9 x 10-8.
- Find the ClO- concentration of a mixture that is 0.300 M in HF and 0.150 M in HClO.
- The Ka of HClO is 3.0x 10^-8 at 25 deg C. What is the percent ionization of HClO in a 0.015M aqueous solution of HCLO at 25 deg C?
- Use the Henderson?Hasselbalch equation to calculate the pH of each solution: a) a solution that is 0.115 M in HClO and 0.170 M in KClO b) a solution that contains 1.45% C2H5NH2 by mass and 1.06% C2H5N
- The Ka of hypochlorous acid (HClO) is 3.0 x 10-8 at 25 deg C. Calculate the pH of a 0.385 M hypochlorous acid solution. a) 3.05 b) 9.53 c) 4.47 d) 6.52 e) -3.05
- Calculate the equilibrium constant for the weak acid HClO, if a solution of the acid with an initial concentration of 7.36 * 10-1 M has a [OCl-] of 0.000160 M (make an exact calculation assuming that
- Calculate the pH of a 4.22x10-4 M solution of the weak acid HClO (Make an exact calculation assuming that initial concentration is not equal to the equilibrium concentration). Round your answer to 3 significant digits. HClO \rightleftharpoons OCl- + H+
- What is the ph of a 0.10 M NaClO solution ? ka for HClO is 3.0x10-8
- The acid-dissociation constant for hypochlorous acid (HClO) is 3.0 x 10-8. Calculate the concentration of H3O+, ClO-, and HClO at equilibrium if the initial concentration of HClO is 7.8 x 10-3.
- Calculate the (OCl-) of a 6.35 x 10-3 M solution of the weak acid HClO (make an exact calculation assuming the initial concentration is not equal to the equilibrium concentration). HClO arrow OCl- + H+; Ka = 3.50 x 10-8
- What is the fraction of HClO in a solution with pH 7.00, where Cl2(aq) reacts with 2 H2O(l) to produce HClO(aq), H3O+(aq), and Cl-(aq)? The Ka of HClO is 2.9 * 10^-8 and the fraction of HClO is defined as (HClO)/((HClO) + (ClO-)). Additionally, what is th
- The Ka for hypochlorous acid (HClO) is 3.5 times 10^8. What is the pH of a 1.50M solution? A. 11.3 B. 5.1 C. 4.3 D. 3.6 E. 1.8
- Which solution will have the lowest pH? a. 0.10 M HClO_2, pK_a = 1.96. b. 0.10 M HCN, pK_a = 9.21. c. 0.10 M HF, pK_a = 3.19. d. 0.10 M HClO, pK_a = 7.538. e. 0.00010 M HCl.
- The Ka for hypochlorous acid (HClO) is 3.0 x 10-8. What is (OH-) in a 0.45 M solution of sodium hypochlorite (NaClO)?
- Find the pH of a 0.0075 M aqueous solution of hypochlorous acid (HClO), for which Ka = 3.5 x 10-8. A. 1.25 B. 3.28 C. 1.17 D. 4.79 E. 1.64
- A solution is prepared by dissolving 0.600 mol of hypochlorous acid and 0.266 mol of nitrous acid in water and diluting to 3.80 L. Calculate the equilibrium molar concentration of HClO.
- What is the value of Ka for HClO, given that a 0.10 M solution has a pH of 4.27?
- What is the pH of a 0.95 M solution of HClO? (Ka = 2.9 x 10-8)
- What is the pH of a 0.530 M solution of HClO? (Ka = 2.9 x 10-8)
- What is the pH of a 0.0137 M solution of HClO with ka = 3.0*10^-8?
- What is the pH of a 0.0157 M solution of HClO? (Ka = 3.0 x 10-8)
- What is the pH of a 0.35 M solution of HClO? (Ka = 2.9 x 10-8)
- Find the pH of a solution that contains 0.044 M HClO and 0.062 M NaClO. The acid dissociation constant of hypochlorous acid is 2.9 times 10^-8.
- The Ka of hypochlorous acid (HClO) is 3.00 x 10-8 at 25.0 degrees C. Calculate the pH of a 0.0385 M hypochlorous acid solution. a. 1.41 b. 7.52 c. -1.41 d. 4.47 e. 8.94
- Hypochlorous acid, HClO, has a pKa of 7.54. What are [H+_O^+], pH, [ClO^-], and [HClO] in 0.137 M HClO?
- Hypochlorous acid, HClO, has a pK_a of 7.54. What are [H_3O^+], pH, [ClO^-], and [HClO] in 0.151 M HClO?
- Hypochlorous acid, HClO, has a pKa of 7.54. What are [H_3O^+], pH, [ClO^-], and [HClO] in 0.145 M HClO?
- A buffer solution is 0.452 M in HClO and 0.313 M in NaClO. If Ka for HClO is 3.5 x 10-8, what is the pH of this buffer solution?
- A buffer solution is 0.465 M in HClO and 0.269 M in NaClO. If Ka for HClO is 3.5 x 10^-8, what is the pH of this buffer solution?
- A buffer solution is made that is 0.469 M in HClO and 0.469 M in KClO. If the Ka for HClO is 3.50 x 10-8, what is the pH of the buffer solution?
- The acid-dissociation constant for hypochlorous acid (HClO) is 3.0\times10-8. Part A Calculate the concentration of H3O+ at equilibrium if the initial concentration of HClO is 8.6\times10^{-3} M .
- The acid-dissociation constant for hypochlorous acid (HClO) is 3.0 * 10-8. Part A Calculate the concentration of H3O+ at equilibrium if the initial concentration of HClO is 6.9 * 10^-3M . Express
- What is the Ka of a 0.80 M HClO solution whose pH is 3.81?
- What is constitutes a buffer solution? What is the % ionization of hypochlorous acid HCLO in a 0.015 M aqueous solution of HCLO at 25 degree C? K= 3.0 times 10^{-8})
- Calculate the (H+) of 25 mL of 0.10 M HClO4 and 25 mL of 0.15 M HClO (Ka = 2.9 x 10-8).
- What is the pH of a mixture of 0.150 M HCHO2 and 0.100 M HClO? The Ka of HCHO2 is 1.8 x 10-4 and 2.9 x 10-8 for HClO.
- Calculate the concentration of all the species present in a 0.100 M solution of hypoiodous acid. (Ka = 2.3 x 10-11)
- Find the pH of a 0.265 M KClO solution. (The K_a of hypochlorous acid, HClO, is 2.0 x 10^-8.)
- Use the Henderson-Hasselbalch equation to calculate the pH of a solution that is 0.135 M in HClO and 0.150 M in KClO.
- Use the Henderson-Hasselbalch equation to calculate the pH of a solution that is 0.165 M in HClO and 0.185 M in KClO.
- What is the pH of a solution that contains 2.0 M HClO and 2.0 M NaClO? K_a of HOCl = 2.9 times 10^{-8}.
- A 100.0 mL buffer solution is 0.185 M in HClO (pKa = 7.54) and 0.160 M in NaClO. What is the pH of the solution?
- Calculate the pH of a hypochlorite buffer containing .150M HCLO and .100M NaCLO.
- Calculate the pH of a hypochlorite buffer containing 0.150 M HClO and 0.100 M NaClO.
- Calculate the pH of a buffer that is 0.158 M HClO and 0.099 M NaClO. The K_a for HClO is 2.9 times 10^{-8}.
- Calculate the pH of a buffer that is 0.158 M HClO and 0.999 M NaClO. The K_a for HClO is 2.9 times 10^{-8}. a. 7.54. b. 6.67. c. 3.77. d. 6.46. e. 7.33.
- Use the Henderson - Hasselbalch equation to calculate the pH of each solution a solution that is 0.135 M in HClO and 0.180 M in KClO a solution that contains 1.47% C_2H_5NH_2 by mass and 1.50% by mas
- The Ka of hypochlorous acid (HClO) is 3.0 x 10-8 at 25.0 degrees Celsius. What is the % ionization of hypochlorous acid in a 0.015 M aqueous solution of HClO at 25.0 degrees Celsius?
- What is the pH of a 0.100 M hypochlorous acid solution? The Ka of HClO is 3.5 x 10-8. a) 3.72 b) 3.23 c) 4.72 d) 4.23 e) 5.08
- The acid-dissociation constant for hypochlorous acid (HClO) is 3.0 times 10^{-8}. Calculate the concentration of H_3O^+ at equilibrium if the initial concentration of HClO is 8.3.
- Find the pH of a 0.250 M NaCIO solution. The acid constant of hypochlorous acid, HClO, is Ka = 2.9 x 10-8.
- The K_a \text{ of hypochlorous acid (HClO) is } 3.00 \times 10^{-8} \text{ at } 25.0^oC. Calculate the pH of a 0.0385 M hypochlorous acid solution. A.1.41 B.7.52 C.-1.41 D.4.47 E.8.94
- Calculate the concentrations of all species in a 0.390 M Na_2SO_3 (sodium sulfite) solution. The ionization constants for sulfurous acid are K_{a1} = 1.4 times 10^{- 2}and K_{a2} = 6.3 times 10^{-8}.
- The ionization constant for hypochlorous acid (HClO) is K_a= 2.8 times 10^{-8} at T= 25 degrees C. Find the pH for an aqueous solution that is 0.0500 M in HClO.
- A buffer solution is 0.383 M in HClO and 0.258 M in KClO. If Ka for HClO is 3.5 x 10^{-8}, what is the pH of this buffer solution?
- Calculate the concentrations of all species in a 1.67 M Na_2SO_3 (sodium sulfite) solution. The ionization constants for sulfurous acid are K_{a1} = 1.4 times 10 ^{-2} and K_{a2} = 6.3 times 10^{- 8}.
- A solution of 0.10 M NaClO is created. The K_a of the conjugate acid (HClO) is 3.0 \times 10^{-8}. Determine the pH of this solution.
- What is the pH of 0.50 M HCl_O? K_a of HCl_O is 3.5 \times 10^{-8}
- Write the Ka expression for HClO in water
- Calculate the concentrations of all of the species in a 0.83 M K_2SO_3 solution. The ionization constants for sulfurous acid are K_{a1} = 1.4 times 10^{-2} and K_{a2} = 6.3 times 10^{-8}. A. (K^+). B. (SO_3^{2-}). C. (HSO_3^-). D. (H_2SO_3). E. (OH^-). F.