## What is the pH of a 2.8 M solution of HClO4?

Therefore pH of 2.8 M HClO4 solution is **-0.45** .

## What is the pH of a 1.4 M solution of HClO4?

**-0.15**. Perchloric acid or HClO4 is a strong acid.

## What is the pH of 1.8 m HClO4?

The value of Ho for 1.8 M HClO4 is **-0.58** somewhat stronger than the value predicted from -log(1.8) = -0.26.

## What is the pH of a 3.0 M solution of HClO4?

pH is defined as the negative log of hydrogen or hydronium ion concentration. Thus pH of 1.34 × 10−3 M HClO4 is **2.87**.

## What is the pH of a 1.7 M solution of HClO4 pH?

**0.23**.

## How do you calculate pH from molarity of HClO4?

**1 Answer**

- We use the pH equation which states that
- pH=−log[H+]
- And so the pH will be
- pH=−log[0.075]
- ≈1.12.

## What is the pH of a 0.0045 M solution of HClO4?

**2.49**| Chegg.com.

## What is the pH of Ca Oh 2?

Base | Name | 100 mM |
---|---|---|

Ca(OH)_{2} |
calcium hydroxide (lime CaO:H_{2}O) |
12.46 |

CaCO_{3} |
calcium carbonate (calcite) | 9.91 |

Cd(OH)_{2} |
cadmium hydroxide | 9.36 |

Co(OH)_{2} |
cobalt(II) hydroxide | 9.15 |

## What is the pH of a 0.1 M solution of HCN?

**5.2**.

## What is the pH of a .001 M Ca Oh 2?

So the concentration of OH- ions in the solution is 0.1M.So pOH is 1 and hence pH is **13**.

## What is the pH of a 0.033 M KOH solution?

pH = 14 – pOH = 14 – 1.48 = **12.52**. Therefore the pH of a 0.033 M KOH solution would be 12.52.

## What is the pH of 0.0333 M hno3 is the solution neutral acidic or basic?

Hence 0.0333 M HNO_{3} is **acidic**.

## Is HClO4 a strong acid?

The 7 common **strong** acids are: HCl HBr HI HNO3 HClO3 HClO4 and H2SO4 (1st proton only). … This means the conj base of HCl the Cl- anion is an extremely weak base and in fact does not act as a base in water (gives a neutral solution).

## What is the pH of perchloric acid?

**1.55**. The pH of an acid can be calculated by taking the negative log of the hydrogen ion concentration in…

## What is the pH of a NaOH solution?

**13**.

## What is the pH of a 0.0075 M solution of HCL?

Mike Schuck · Ernest Z. The pH is **1.60**.

## What is the pH of a 0.050 M LiOH solution?

The answer is: e. **12.70** pOH = -log[OH-] = -log[LiOH] =…

## What is the pOH of a 50.0 ml solution of 0.050 M HClO4?

1 Expert Answer

If pH is 1.3 pOH will be **12.7**.

## What is the Ka of HClO4?

Ka | Acid | |
---|---|---|

Name | Formula | |

Large | Perchloric acid | HClO_{4} |

3.2 * 10^{9} |
Hydroiodic acid | HI |

1.0 * 10^{9} |
Hydrobromic acid | HBr |

## How do you convert pH to Ka?

As noted above [H3O+] = 10^{–}^{pH}. Since x = [H3O^{+}] and you know the pH of the solution you can write x = 10^{–}^{2.4}. It is now possible to find a numerical value for Ka. **Ka = (10 ^{–}^{2.4})**

^{2}/(0.9 – 10

^{–}

^{2.4}) = 1.8 x 10

^{–}

^{5}.

## What is the pH of hydrochloric acid solution?

**1.5 to 3.5**. A weak acid or base does not ionize completely in aqueous solution. Ionization of a weak acid (HA) is characterized by its dissociation constant (K

_{a}).

## Can you have a negative pH?

**any acid that yields a concentration of hydrogen ions with a molarity greater than 1 will be calculated to have a negative pH**. For example the pH of 12M HCl (hydrochloric acid) is calculated to be -log(12) = -1.08.

## What is the pH of an aqueous 0.0104 M Ca OH 2 solution?

Question: what is the pH of a 0.014 M Ca(OH)2 solution? the answer is supposed to be **12.45** but i keep getting12.

## Is Ca Oh 2 an acid?

**base**.

## What is the pH of a 0.015 M Ca OH 2 solution?

**12.48**.

## What is the pH of a 0.02 M solution of sodium hydroxide?

pH of 0.02M of NaOH is **12.30**.

## What is the pH value of 0.02 m NaOH solution?

Its concentration here is high enough to ignore H3O+ contribution from water so the pH is just -log(0.02) = **1.7**. pH + pOH = 14 so the pOH is 12.3.

## What is the pH of a 0.02 M sodium hydroxide solution is sodium hydroxide an acid or a base?

The pH of the solution is **12.3**. Because sodium hydroxide is a strong base it makes sense that the pH is above 7.

## What is the pOH of a 0.02 M Ca OH 2 solution?

….for calcium hydroxide we got [HO−]=0.04⋅mol⋅L−1 … …and so pOH=−log10(0.04)=−(−1.40)=**1.40** …

## How do you find the pH of a solution?

To calculate the pH of an aqueous solution you need to know the concentration of the hydronium ion in moles per liter (molarity). The pH is then calculated using the expression: **pH = – log [H _{3}O^{+}].**

## What is the pH of a 0.005 M Ca OH 2 solution?

**12**.

## What is the pH solution of 0.003 M?

**2.52**and pOH is 11.48.

## What is the pH of 0.1 M KOH?

If concentration of KOH is 0.1 M pH value may be **13**. If concentation is 0.0001 M pH value will be 10. Therefore pH range of KOH solution will be 10-13.

## What is the pH of 0.25 M KOH?

We’re being asked to calculate the pH of a 0.25 M KOH solution. The pH of the solution is **13.4**.

## What is the pH of a 0.050 M HBr solution?

## How to Calculate the pH of a Solution

## pH pOH H3O+ OH- Kw Ka Kb pKa and pKb Basic Calculations -Acids and Bases Chemistry Problems

## Calculate the pH of an Acidic Salt (Ammonium Chloride)